KR101871950B1 - Hydrogen-Catalyst Reactor - Google Patents

Abstract

A reaction cell for the catalysis of atomic hydrogen, a hydrogen atom source, at least one reactant comprising elements or elements that form a catalyst, and at least one A source of hydrogen catalyst comprising a reaction mixture with other elements is provided whereby a catalyst is formed from the source and the catalytic action of the atomic hydrogen releases an energy of greater than about 300 kJ per mole of hydrogen during the catalysis of atomic hydrogen .

Description

A hydrogen-catalytic reactor (Hydrogen-Catalyst Reactor)

Cross-reference to related application

The Applicant claims the benefit of and is incorporated herein by reference in its entirety:

(1) Application No. 60 / 913,556 filed on April 24, 2007; (2) Application No. 60 / 952,305 filed on July 27, 2007; (3) Application No. 60 / 954,426 filed on August 7, 2007; (4) Application No. 60 / 935,373 filed on August 9, 2007; (5) Application No. 60 / 955,465 filed on August 13, 2007; (6) Application No. 60 / 956,821 filed on August 20, 2007; (7) Application No. 60 / 957,540 filed on August 23, 2007; (8) Application No. 60 / 972,342 filed on September 14, 2007; (9) Application No. 60 / 974,191 filed on September 21, 2007; (10) Application No. 60 / 975,330 filed on September 26, 2007; (11) Application No. 60 / 976,004 filed on September 28, 2007; (12) Application No. 60 / 978,435 filed on October 9, 2007; (13) Application No. 60 / 987,552 filed on November 13, 2007; (14) Application No. 60 / 987,946 filed on November 14, 2007; (15) Application No. 60 / 989,677 filed on November 21, 2007; (16) Application No. 60 / 991,434 filed on November 30, 2007; (17) Application No. 60 / 991,974 filed on December 3, 2007; (18) Application No. 60 / 992,601 filed on December 5, 2007; (19) Application No. 61 / 012,717 filed on December 10, 2007; (20) Application No. 61 / 014,860 filed on December 19, 2007; (21) Application No. 61 / 016,790 filed on December 26, 2007; (22) Application No. 61 / 020,023 filed on January 9, 2008; (23) Application No. 61 / 021,205 filed on January 15, 2008; (24) Application No. 61 / 021,808 filed on January 17, 2008; (25) Application No. 61 / 022,112 filed on January 18, 2008; (26) Application No. 61 / 022,949 filed on January 23, 2008; (27) Application No. 61 / 023,297 filed on January 24, 2008; (28) Application No. 61 / 023,687 filed on January 25, 2008; (29) Application No. 61 / 024,730 filed on January 30, 2008; (30) Application No. 61 / 025,520 filed on February 1, 2008; (31) Application No. 61 / 028,605 filed on February 14, 2008; (32) Application No. 61 / 030,468 filed on February 21, 2008; (33) Application No. 61 / 064,453 filed on March 6, 2008; (34) Application No. 61 / xxx, xxx filed on March 21, 2008, and (35) Application No. 61 / xxx, xxx filed on April 17, 2008.

Invention of the invention

1. Field of the Invention

(p≤137이 정수임)이 수소 여기 상태를 위한 리드베리 방정식에서 잘 알려진 변수인 n=정수를 대체한다. He⁺, Ar⁺ 및 K는 촉매로서 기능할 것으로 예측되는데, 왜냐하면 이들의 화학 또는 물리적 공정의 엔탈피 변화가 수소 원자의 포텐셜 에너지인 27.2eV의 정수배와 같아서, 촉매 조건(catalyst criterion)을 충족시키기 때문이다. 에너지 준위에 관한 닫힌 형태(closed-form) 방정식에 근거한 특정 예측들을 시험하였다. 예를 들면, 두 개의 H(1/p)은 반응하여, 촉매화되지 않은 수소 원자를 포함하는 H₂의 P²배의 진동 및 회전 에너지를 갖는 H₂(1/p)을 형성할 수 있다. 대기압 전자빔 여기 아르곤-수소 플라즈마로부터 145-300 nm 영역에서 회전선들이 관찰되었다. 수소의 4²배의 전례가 없는 에너지 간격(spacing)이 핵간 거리가 H₂의 (1/4)임을 입증하였고, 임을 확인하였다.* Paper, which is incorporated herein by reference, R. Mills, J. He, Z. Chang, W. Good, Y. Lu, B. Dhandapani, "Catalysis of Atomic Hydrogen to Novel Hydrogen Species H - (1/4 ) and H ₂ (1/4) as a New Power Source ", Int. J. Hydrogen Energy, Vol. 32, No. 12, (2007), pp. As disclosed in 2573-2584, data from a wide range of investigation techniques suggests that hydrogen can exist in a low-energy state that was previously thought to be possible in a strong and consistent manner. The predicted response involves transmitting resonant, non-radiative energy from a stable hydrogen atom to a catalyst capable of receiving energy. The product is H (1 / p), which is the Rydberg fractional state of the hydrogen atom,

(p? 137 is an integer) replaces the well-known variable n = integer in the Reed-Berry equation for the hydrogen-excited state. He ⁺ , Ar ^+, and K are expected to function as catalysts because their enthalpy change in the chemical or physical process is equal to an integral multiple of 27.2 eV, the potential energy of the hydrogen atom, satisfying the catalyst criterion to be. Specific predictions based on closed-form equations for energy levels were tested. For example, two H (1 / p) may react to form H ₂ (1 / p) with a vibration and rotational energy of P ² times H ₂ containing un-catalyzed hydrogen atoms . Rotational lines were observed in the region of 145-300 nm from atmospheric pressure electron beam excited argon - hydrogen plasma. It has been verified that an unprecedented spacing of 4 ² times the hydrogen proves that the intercritical distance is (1/4) of H ₂ .

The product of the predicted alkali catalyst K is H ^- (1/4) capable of forming a new alkaline halide (X) hydride compound, KH * X, and H ₂ (1/4) to be. The 1H MAS NMR spectrum of the novel compound KH * Cl versus the external tetramethylsilane (TMS) showed a large and distinct upfield resonance at -4.4 ppm, corresponding to an absolute resonance shift of -35.9 ppm, This is consistent with the theoretical predictions of H ^- (1 / p) with p = 4. The frequencies of the predicted ortho and para-H ₂ (1/4) are 1943 cm ^-1 and 2012 cm ^-1 in the high-resolution FTIR spectrum of KH * I with a -4.6 ppm NMR peak assigned to H ^- (1/4) Respectively. The 1943/2012 cm-1-intensity ratio was consistent with the characteristic 3: 1 ortho: para-peak-intensity ratio, and the ortho-para splitting at 69 cm ^-1 was consistent with the predicted. By NMR, KH * Cl with H ^- (1/4) was common to the 12.5 KeV electron beam, which excited a similar emission of the gap H ₂ (1/4), as observed in an argon-hydrogen plasma. KNO ₃ and Raney nickel were used as sources of K catalyst and atomic hydrogen, respectively, to generate the corresponding exothermic reaction. The energy balance was ΔH = -17,925 kcal / mole KNO ₃ , which is about 300 times that expected, due to combustion between hydrogen and atmospheric oxygen, the KNO ₃ chemical reaction being known to be the most intense, and the theoretical maximum enthalpy of -57.8 kcal / mole H ₂ , which was more than 60 times that of -3585 kcal / mole H ₂ . The reduction process of KNO ₃ to water, potassium metal and NH ₃ , calculated from the heat of generation, emitted only -14.2 kcal / mole H ₂ , which can not account for observed heat or hydrogen combustion. However, these results are consistent with the formation of H ^- (1/4) and H ₂ (1/4) with a production enthalpy over 100 times that of combustion.

In embodiments, the invention includes a power source and a reactor that form low energy hydrogen species and compounds. The present invention further comprises a catalyst and a reaction mixture which provides atomic hydrogen. Preferred atomic catalysts are lithium, potassium, and cesium atoms. A preferred molecular catalyst is NaH.

Hydrino

The given binding energy

(1)

(One)

(p is an integer greater than 1, preferably between 2 and 137) is disclosed in the following references:

RL Mills, " The Grand Unified Theory of Classical Quantum Mechanics ", October 2007 Edition, (posted at http://www.blacklightpower.com/theory/book.shtml); Black Mill Power, Inc., 493 Old Trenton Road, Cranbury, NJ, 08512 (posted at www.blacklightpower.com), R. Mills, The Grand Unified Theory of Classical Quantum Mechanics, May 2006 Edition, BlackLight Power, Inc ., Cranbury, New Jersey, ("'06 Mills GUT "); R. Milles, The Grand Unified Theory of Classical Quantum Mechanics, January 2004 Edition, BlackLight Power, Inc., Cranbury, New Jersey, (" 04 Mills GUT "); BlackLight Power, Inc., Cranbury, New Jersey, (" R. Mills, " The Grand Unified Theory of Classical Quantum Mechanics, September 2003 Edition, provided by BlackLight Power, Inc., 493 Old Trenton Road, Cranbury, NJ, 03 Mills GUT "); The Grand Unified Theory of Classical Quantum Mechanics, September 2002 Edition, BlackLight Power, Inc., Cranbury, New Jersey, (" R.Mills ", supplied by BlackLight Power, Inc., 493 Old Trenton Road, Cranbury, NJ, 02 Mills GUT "); R. Mills, The Grand Unified Theory of Classical Quantum Mechanics, September 2001 Edition, BlackLight Power, Inc., Cranbury, New Jersey, Distributed by Amazon, provided by BlackLight Power, Inc., 493 Old Trenton Road, Cranbury, NJ, 08512 .com ("'01 Mills GUT"); R. Mills, The Grand Unified Theory of Classical Quantum Mechanics, January 2000 Edition, BlackLight Power, Inc., Cranbury, New Jersey, Distributed by Amazon, provided by BlackLight Power, Inc., 493 Old Trenton Road, Cranbury, NJ, 08512 .com ("'00 Mills GUT"); RL Mills, " Physical Solutions of the Nature of the Atom, Photon, and Their Interactions to Form Excited and Predicted Hydrino States, " Physics Essay, inpress; RL Mills, " Exact Classical Quantum Mechanical Solution for Atomic Helium, " which Predicts Conjugate Parameters from a Unique Solution for the First Time, " Physics Essays, inpress; RL Mills, P. Ray, B. Dhandapani, " Excessive Balmer Line Broadening of Water-Vapor Capacitively-Coupled RF Discharge Plasmas, " International Journal of Hydrogen Energy, Vol. 33, (2008), 802-815; RL Mills, J. He, M. Nansteel, B. Dhandapani, " Catalysis of Atomic Hydrogen to New Hydrides as a New Power Source, " RL Mills, H. Zea, J. He, B. Dhandapani, " Water Bath Calorimetry on a Catalytic Reaction of Atomic Hydrogen, " J. Phillips, CK Chen, RL Mills, " Evidence of Catalytic Hydrogen in RF-Generated Hydrogen / Argon Plasmas, " RL Mills, J. He, Y. Lu, M. Nansteel, Z. Chang, B. Dhandapani, "Comprehensive Identification and Potential Applications of New States of Hydrogen," Int. J. Hydrogen Energy, Vol. 32 (14), (2007), 2988-3009; RL Mills, J. He, Z. Chang , W. Good, Y. Lu, B. Dhandapani, "Catalysis of Atomic Hydrogen to Novel Hydrogen Species H - (1/4) and H 2 (1/4) as a New Power Source, " Int. J. Hydrogen Energy, Vol. 32 (13), (2007), pp. 2573-2584; RL Mills, " Maxwell ' s Equations and QED: Physics Essays, Vol. 19, (2006), 225-262; RL Mills, P. Ray, B. Dhandapani, Evidence of an energy transfer reaction between atomic hydrogen and argon II or helium II, J. Plasma Physics, Vol. 72, No. 4, (2006), 469-484; RL Mills, " Exact Classical Quantum Mechanical Solutions for One-through Twenty-Electron Atoms, " Physics Essays, Vol. 18, (2005), 321-361; RL Mills, PC Ray, RM Mayo, M. Nansteel, B. Dhandapani, J. Phillips, "Spectroscopic Study of Unique Line Broadening and Inversion in Microwave Generated Water Plasmas," J. Plasma Physics, Vol. 71, No. 6, (2005), 877-888; RL Mills, "The Fallacy of Feynman's Argument on the Stability of the Hydrogen Atom According to Quantum Mechanics," Ann. Fund. Louis de Broglie, Vol. 30, No. 2, (2005), pp. 129-151; RL Mills, B. Dhandapani, J. He, "Highly Stable Amorphous Silicon Hydride from a Helium Plasma Reaction," Materials Chemistry and Physics, 94 / 2-3, (2005), 298-307; RL Mills, J. He, Z. Chang, W. Good, Y. Lu, B. Dhandapani, "Catalysis of Atomic Hydrogen to Novel Hydrides as a New Power Source," Prepr. Pap.Am. Chem. Soc. Conf., Div. Fuel Chem., Vol. 50, No. 2, (2005); RL Mills, J. Sankar, A. Voigt, J. He, P. Ray, B. Dhandapani, "Role of Atomic Hydrogen Density and Energy in Low Power CVD Synthesis of Diamond Films," Thin Solid Films, 77-90; RL Mills, " The Nature of the Chemical Bond Revisited and an Alternative Maxwellian Approach, " Physics Essays, Vol. 17, (2004), 342-389; RL Mills, P. Ray, "Stationary Inverted Lyman Population and a Very Stable Novel Hydride Formed by a Catalytic Reaction of Atomic Hydrogen and Certain Catalysts," J. Opt. Mat., 27, (2004), 181-186; W. Good, P. Jansson, M. Nansteel, J. He, A. Voigt, " Spectroscopic and NMR Identification of Novel Hydride Ions in Fractional Quantum Energy States for an Exothermic Reaction of Atomic Hydrogen with Certain Catalysts, : Applied Physics, 28, (2004), 83-104; J. Phillips, RL Mills, X. Chen, " Water Bath Calorimetric Study of Excess Heat in Resonance Transfer " Plasmas, J. Appl. Phys., Vol. 96, No. 6, (2004) 3095-3102; RL Mills, Y. Lu, M. Nansteel, J. He, A. Voigt, W. Good, B. Dhandapani, "Energetic Catalyst-Hydrogen Plasma Reaction as a Potential New Energy Source," Division of Fuel Chemistry, in Hydrogen Energy, Prepr. Pap.Am. Chem. Soc. Conf., Vol. 49, No. 2, (2004); RL Mills, J. Sankar, A. Voigt, J. He, B. Dhandapani, "Synthesis of HDLC Films from Solid Carbon," J. Materials Science, J. Mater. Sci. 39 (2004) 3309-3318; RL Mills, Y. Lu, M. Nansteel, J. He, A. Voigt, B. Dhandapani, "Energetic Catalyst-Hydrogen Plasma Reaction as a Potential New Energy Source," Division of Fuel Chemistry, Session: , and Gaseous Fuels, Prepr. Pap.Am. Chem. Soc. Conf., Vol. 49, No. 1, (2004); RL Mills, " Classical Quantum Mechanics, " Physics Essays, Vol. 16, (2003), 433-498; RL Mills, P. Ray, M. Nansteel, J. He, X. Chen, A. Voigt, B. Dhandapani, "Characterization of an Energetic Catalyst-Hydrogen Plasma Reaction as a Potential New Energy Source," Am. Chem. Soc. Div. Fuel Chem. Prepr., Vol. 48, No. 2, (2003); RL Mills, J. Sankar, A. Voigt, J. He, B. Dhandapani, "Spectroscopic Characterization of Atomic Hydrogen Energies and Densities and Carbon Species During Helium-Hydrogen-Methane Plasma CVD Synthesis of Diamond Films," Chemistry of Materials, Vol. 15, (2003), pp. 1313-1321; RL Mills, P. Ray, " Extreme Ultraviolet Spectroscopy of Helium-Hydrogen Plasma, " J. Phys. D, Applied Physics, Vol. 36, (2003), pp. 1535-1542; RL Mills, X. Chen, P. Ray, J. He, B. Dhandapani, "Plasma Power Source Based on a Catalytic Reaction of Atomic Hydrogen Measured by Water Bath Calorimetry," Thermochimica Acta, Vol. 406 / 1-2, (2003), pp. 35-53; RL Mills, B. Dhandapani, J. He, "Highly Stable Amorphous Silicon Hydride," Solar Energy Materials & Solar Cells, Vol. 80, No. 1, (2003), pp. 1-20; RL Mills, P. Ray, RM Mayo, " The Potential for a Hydrogen Water-Plasma Laser, " Applied Physics Letters, Vol. 82, No. 11, (2003), pp. 1679-1681; RL Mills, P. Ray, " Stationary Inverted Lyman Population Formed from Incandescently Heated Hydrogen Gas with Certain Catalysts, " J. Phys. D, Applied Physics, Vol. 36, (2003), pp. 1504-1509; RL Mills, P. Ray, B. Dhandapani, J. He, "Comparison of Excessive Balmer α Line Broadening of Inductively and Capacitively Coupled RF, Microwave, and Glow Discharge Hydrogen Plasmas with Certain Catalysts," IEEE Transactions on Plasma Science, Vol. 31, No. (2003), pp. 338-355; RL Mills, P. Ray, RM Mayo, " CW HI Laser Based on a Stationary Inverted Lyman Population Formed from Incandescently Heated Hydrogen Gas with Certain Group I Catalysts, " IEEE Transactions on Plasma Science, Vol. 31, No. 2, (2003), pp. 236-247; RL Mills, P. Ray, J. Dong, M. Nansteel, B. Dhandapani, J. He, "Spectral Emission of Fractional-Principal-Quantum-Energy-Level Atomic and Molecular Hydrogen," Vibrational Spectroscopy, Vol. 31, No. 2, (2003), pp. 195-213; H. Conrads, RL Mills, Th. Wrubel, " Emission in the Deep Vacuum Ultraviolet from a Plasma Formed by Incandescent Heating Hydrogen Gas with Trace Amounts of Potassium Carbonate, " Plasma Sources Science and Technology, Vol. 12, (2003), pp. 389-395; RL Mills, J. He, P. Ray, B. Dhandapani, X. Chen, " Synthesis and Characterization of a Highly Stable Amorphous Silicon Hydride as the Product of a Catalytic Helium-Hydrogen Plasma Reaction, J. Hydrogen Energy, Vol. 28, No. 12, (2003), pp. 1401-1424; RL Mills, P. Ray, "A Comprehensive Study of Spectra of the Bound-Free Hyperfine Levels of Novel Hydride Ion H - (1/2), Hydrogen, Nitrogen, and Air," Int. J. Hydrogen Energy, Vol. 28, No. 8, (2003), pp. 825-871; RL Mills, M. Nansteel, and P. Ray, "Excessively Bright Hydrogen-Strontium Plasma Light Source Due to Energy Resonance of Strontium with Hydrogen," J. Plasma Physics, Vol. 69, (2003), pp. 131-158; RL Mills, " Highly Stable Novel Inorganic Hydrides, " J. New Materials for Electrochemical Systems, Vol. 6, (2003), pp. 45-54; RL Mills, P. Ray, " Substantial Changes in a Microwave Plasma Due to Combining Argon and Hydrogen, " New Journal of Physics, www.njp.org, Vol. 4, (2002), pp. 22.1-22.17; RM Mayo, RL Mills, M. Nansteel, "Direct Plasmadynamic Conversion of Plasma Thermal Power to Electricity," IEEE Transactions on Plasma Science, October, (2002), Vol. 30, No. 5, pp. 2066-2073; RL Mills, M. Nansteel, P. Ray, " Bright Hydrogen-Light Source Due to a Resonant Energy Transfer with Strontium and Argon Ions, " New Journal of Physics, Vol. 4, (2002), pp. 70.1-70.28; RM Mayo, RL Mills, M. Nansteel, "On the Potential of Direct and MHD Conversion of Power from a Novel Plasma Source to Electricity for Microdistributed Power Applications," IEEE Transactions on Plasma Science, August, (2002), Vol. 30, No. 4, pp. 1568-1578; RM Mayo, RL Mills, "Direct Plasmadynamic Conversion of Plasma Thermal Power to Electricity for Microdistributed Power Applications," 40th Annual Power Sources Conference, Cherry Hill, NJ, June 10-13, (2002), pp. 1-4; RL Mills, E. Dayalan, P. Ray, B. Dhandapani, J. He, "Highly Stable Novel Inorganic Hydrides from Aqueous Electrolysis and Plasma Electrolysis," Electrochimica Acta, Vol. 47, No. 24, (2002), pp. 3909-3926; RL Mills, P. Ray, B. Dhandapani, RM Mayo, J. He, "Comparison of Excessive Balmer α Line Broadening of Glow Discharge and Microwave Hydrogen Plasmas with Certain Catalysts," J. of Applied Physics, Vol. 92, No. 12, (2002), pp. 7008-7022; RL Mills, P. Ray, B. Dhandapani, M. Nansteel, X. Chen, J. He, "New Power Source from Fractional Quantum Energy Levels of Atomic Hydrogen that Surpasses Internal Combustion," J. Mol. Struct., Vol. 643, No. 13, (2002), pp. 43-54; RL Mills, J. Dong, W. Good, P. Ray, J. He, B. Dhandapani, "Measurement of Energy Balances of Noble Gas-Hydrogen Discharge Plasmas Using Calvet Calorimetry," Int. J. Hydrogen Energy, Vol. 27, No. 9, (2002), pp. 967-978; RL Mills, P. Ray, " Spectroscopic Identification of a Novel Catalytic Reaction of Rubidium Ion with Atomic Hydrogen and the Hydride Ion Product, " Int. J. Hydrogen Energy, Vol. 27, No. 9, (2002), pp. 927-935; RL Mills, A. Voigt, P. Ray, M. Nansteel, B. Dhandapani, "Measurement of Hydrogen Balmer Linear Broadening and Thermal Power Balances of Noble Gas-Hydrogen Discharge Plasmas," Int. J. Hydrogen Energy, Vol. 27, No. 6, (2002), pp. 671-685; RL Mills, N. Greenig, S. Hicks, " Optically Measured Power Balances of Glow Discharges of Mixtures of Argon, Hydrogen, and Potassium, Rubidium, Cesium, or Strontium Vapor, Int. J. Hydrogen Energy, Vol. 27, No. 6, (2002), pp. 651-670; RL Mills, " The Grand Unified Theory of Classical Quantum Mechanics, " Int. J. Hydrogen Energy, Vol. 27, No. 5, (2002), pp. 565-590; RL Mills, P. Ray, " Vibrational Spectral Emission of Fractional-Principal-Quantum-Energy-Level Hydrogen Molecular Ion, " Int. J. Hydrogen Energy, Vol. 27, No. 5, (2002), pp. 533-564; RL Mills and M. Nansteel, P. Ray, " Argon-Hydrogen-Strontium Discharge Light Source, " IEEE Transactions on Plasma Science, Vol. 30, No. 2, (2002), pp. 639-653; RL Mills, P. Ray, " Spectral Emission of Fractional Quantum Energy Levels of Atomic Hydrogen from a Helium-Hydrogen Plasma and the Implications for Dark Matter, " Int. J. Hydrogen Energy, (2002), Vol. 27, No. 3, pp. 301-322; RL Mills, P. Ray, " Spectroscopic Identification of a Novel Catalytic Reaction of Potassium and Atomic Hydrogen and the Hydride Ion Product, " Int. J. Hydrogen Energy, Vol. 27, No. 2, (2002), pp. 183-192; RL Mills, E. Dayalan, "Novel Alkali and Alkaline Earth Hydrides for High Voltage and High Energy Density Batteries," Proceedings of the 17 th Annual Battery Conference on Applications and Advances, California State University, Long Beach, CA, (January 15- 18, 2002), pp. 1-6; RL Mills, W. Good, A. Voigt, and Jinquan Dong, "Minimum Heat of Formation of Potassium Iodo Hydride," Int. J. Hydrogen Energy, Vol. 26, No. 11, (2001), pp. 1199-1208; RL Mills, " The Nature of Free Electrons in Superfluid Helium-a Test of Quantum Mechanics and a Basis to its Foundations and Make a Comparison to Classical Theory, " Int. J. Hydrogen Energy, Vol. 26, No. 10, (2001), pp. 1059-1096; RL Mills, "Spectroscopic Identification of a Novel Catalytic Reaction of Atomic Hydrogen and the Hydride Ion Product," Int. J. Hydrogen Energy, Vol. 26, No. 10, (2001), pp. 1041-1058; RL Mills, B. Dhandapani, M. Nansteel, J. He, A. Voigt, "Identification of Compounds Containing Novel Hydride Ions by Nuclear Magnetic Resonance Spectroscopy," Int. J. Hydrogen Energy, Vol. 26, No. 9, (2001), pp. 965-979; RL Mills, T. Onuma, and Y. Lu, "Formation of a Hydrogen Plasma from an Incandescently Heated Hydrogen-Catalyst Gas Mixture with an Anomalous Afterglow Duration," Int. J. Hydrogen Energy, Vol. 26, No. 7, July, (2001), pp. 749-762; RL Mills, " Observation of Extreme Ultraviolet Emission from Hydrogen-KI Plasmas Produced by a Hollow Cathode Discharge, " Int. J. Hydrogen Energy, Vol. 26, No. 6, (2001), pp. 579-592; RL Mills, B. Dhandapani, M. Nansteel, J. He, T. Shannon, A. Echezuria, "Synthesis and Characterization of Novel Hydride Compounds," Int. J. of Hydrogen Energy, Vol. 26, No. 4, (2001), pp. 339-367; RL Mills, "Temporal Behavior of Light-Emission in the Visible Spectral Range from a Ti-K2CO3-H-Cell," Int. J. Hydrogen Energy, Vol. 26, No. 4, (2001), pp. 327-332; RL Mills, M. Nansteel, and Y. Lu, " Observation of Extreme Ultraviolet Hydrogen Emission from Incandescent Heated Hydrogen Gas with Strontium That Produced an Anomalous Optically Measured Power Balance, " Int. J. Hydrogen Energy, Vol. 26, No. 4, (2001), pp. 309-326; RL Mills, "BlackLight Power Technology A New Clean Hydrogen Energy Source with the Potential for Direct Conversion to Electricity," Proceedings of the National Hydrogen Association, 12th Annual US Hydrogen Meeting and Exposition, DC, (March 6-8, 2001), pp. 671-697; RL Mills, "The Grand Unified Theory of Classical Quantum Mechanics," Global Foundation, Inc. Orbis Scientiae entitled The Role of Attractive and Repulsive Gravitational Forces in Cosmic Gamma Ray Bursts, (29th Conference on High Energy Physics and Cosmology Since 1964). Behram N. Kursunoglu, Chairman, December 14-17, 2000, Lago Mar Resort, Fort Lauderdale, FL, Kluwer Academic / Plenum Publishers, New York, pp. 243-258; RL Mills, B. Dhandapani, N. Greenig, J. He, " Synthesis and Characterization of Potassium IodoHydride, " Int. 25, Issue 12, December, (2000), pp. 1185-1203; RL Mills, " The Hydrogen Atom Revisited, " Int. J. of Hydrogen Energy, Vol. 25, Issue 12, December, (2000), pp. 1171-1183; RL Mills, "BlackLight Power Technology-A New Clean Energy Source with Potential for Direct Conversion to Electricity," Global Foundation International Conference, "Global Warming and Energy Policy,". Behram. Kursunoglu, Chairman, Fort Lauderdale, FL, November 26-28, 2000, Kluwer Academic / Plenum Publishers, New York, pp. 187-202; RL Mills, J. Dong, Y. Lu, " Observation of Extreme Ultraviolet Hydrogen Emission from Incandescently Heated Hydrogen Gas with Certain Catalysts, " Int. J. Hydrogen Energy, Vol. 25, (2000), pp. 919-943; RL Mills, " Novel Inorganic Hydride, " Int. J. of Hydrogen Energy, Vol. 25, (2000), pp. 669-683; RL Mills, " Novel Hydrogen Compounds from a Potassium Carbonate Electrolytic Cell, " Fusion Technol., Vol. 37, No. " Fractional Quantum Energy Levels of Hydrogen, " Fusion Technology, Vol. 28, No. 4, November, (1995), pp. 1697-1719; RL Mills, W. Good, R. Shaubach, " Dihydrino Molecule Identification, " Fusion Technol., Vol. 25, (1994), 103; RL Mills and S. Kneizys, Fusion Technol. Vol. 20, (1991), 65; And the conventionally published PCT application number. WO 90/13126; WO 92/10838; WO 94/29873; WO 96/42085; WO 99/05735; WO 99/26078; WO 99/34322; WO 99/35698; WO 00/07931; WO 00/07932; WO 01/095944; WO 01/18948; WO 01/21300; WO 01/22472; WO 01/70627; WO 02/087291; WO 02/088020; WO 02/16956; WO 03/093173; WO 03/066516; WO 04/092058; WO 05/041368; WO 05/067678; WO 2005/116630; WO 2007/051078; And WO 2007/053486; And U.S. Patent Nos. 6,024,935 and 7,188,033. The disclosures of which are all incorporated herein by reference ("Mills prior art").

(여기서, aH는 일반적인 수소 원자의 반지름이고 p는 정수임)인 하이드리노에 대한 표시는

이다. 반지름 aH를 갖는 수소 원자는 이하에서 "일반적인 수소 원자" 또는 "정상적인 수소 원자"라고 지칭한다. 일반적인 수소 원자는 결합 에너지가 13.6eV인 것을 특징으로 한다. The binding energy of an atom, ion, or molecule, also known as ionizing energy, is the energy required to remove an electron from an atom, ion, or molecule. The hydrogen atom having the binding energy given in the formula (1) is hereinafter referred to as a hydrino atom or a hydrino. Radius

(Where aH is the radius of a common hydrogen atom and p is an integer)

to be. Hydrogen atoms with radius aH are referred to below as " normal hydrogen atoms " or " normal hydrogen atoms ". A typical hydrogen atom has a binding energy of 13.6 eV.

The hydrino has a general hydrogen atom

m · 27.2 eV (2)

(Where m is an integer) reaction of the catalyst with a net enthalpy of reaction. This catalyst was referred to as a source of energy holes or energy holes in Mills's proposed patent application. The rate of catalysis is believed to increase as the net enthalpy of the reaction is closer to m · 27.2 eV. It has been found that catalysts with a net enthalpy of reaction within ± 10%, preferably within ± 5% of m · 27.2 eV, are suitable for most applications.

This catalytic action releases energy from the hydrogen atom as the size of the hydrogen atom, r _n = na _H , moderately decreases. For example, a catalytic action to H (n = 1) of H (n = 1/2) is released, and a 40.8 eV, hydrogen radius is reduced in a _H to 1/2 _H a. The catalyst system is such that t electrons from one atom are ionized and provided to a continuum energy level, respectively, such that the sum of the ionization energies of the t electrons is approximately m · 27.2 eV (m is an integer).

The one catalyst system comprises lithium metal. The primary and secondary ionization energies of lithium are 5.39172 eV and 75.64018 eV, respectively [1]. The divalent ionization (t = 2) reaction in which Li is Li ²⁺ has a net reaction enthalpy of 81.0319 eV, which is the same as m = 3 in Equation (2).

(3)

(3)

(4)

And the overall reaction is as follows:

(5)

(5)

In another embodiment, the catalyst system comprises cesium. The primary and secondary ionization energies of cesium are 3.89390 eV and 23.15745 eV, respectively. The divalent ionization (t = 2) reaction in which Cs is Cs ²⁺ has a net reaction enthalpy of 27.05135 eV, which is the same as m = 1 in the formula (2).

(6)

(6)

(7)

(7)

And the overall reaction is as follows:

(8)

(8)

Another catalyst system includes potassium metal. The primary, secondary, and tertiary ionization energies of potassium are 4.34066 eV, 31.63 eV, and 45.806 eV [1]. And the trivalent ionization (t = 3) reaction in which K is K ³⁺ has a net reaction enthalpy of 81.7767 eV, which is the same as m = 3 in equation (2).

(9)

(9)

(10)

(10)

The overall reaction is as follows:

(11)

(11)

Like the power source, the energy released during the catalysis is much greater than the energy absorbed by the catalyst. The emission energy is larger than a conventional chemical reaction. For example, when hydrogen and oxygen gas are burned to form water,

(12)

(12)

The known water formation enthalpy is? H _f = -286 kJ / mole or 1.48 eV per hydrogen atom. On the other hand, a typical hydrogen atom (n = 1) undergoing catalysis releases a net enthalpy of 40.8 eV. Moreover, additional catalytic transitions may occur:

등. 일단 촉매작용이 시작되면, 하이드리노는 추가로 불균형(disproportionation)이라 불리는 과정에서 자가촉매작용을 한다. 상기 메커니즘은 무기 이온 촉매작용의 메커니즘과 유사하다. 하지만, 하이드리노 촉매작용은 엔탈피가 m·27.2eV에 더 잘 매치되므로 무기 이온 촉매작용에 비해 반응 속도가 빠르다.

Etc. Once the catalysis is initiated, the hydrino further self-catalyses in a process called disproportionation. The mechanism is analogous to the mechanism of inorganic ion catalysis. However, the hydrinocatalysis has a faster reaction rate than the inorganic ion catalysis because the enthalpy is better matched to m · 27.2 eV.

The additional catalytic products of the present invention

(여기서, n은 1/p이고, p는 1보다 큰 정수임)의 결합 에너지를 갖는 수소 원자와 반응함으로써 형성될 수 있다. 상기 하이드리노 수소화물 이온은 H^-(n=1/p) 또는 H^-(1/p)로 표현된다. The hydrino hydride ion of the present invention is characterized in that the electron source is hydrino,

(Where n is 1 / p and p is an integer greater than 1). The hydrinos hydride ion is represented by H ^- (n = 1 / p) or H ^- (1 / p).

(13)

(13)

(14)

(14)

The hydrino hydride ions are distinguished from common hydride nuclei and common hydride ions containing two electrons with a binding energy of about 0.8 eV. The latter is referred to below as " normal hydride ion " or " normal hydride ion ". The hydrino hydride ion contains two indistinguishable electrons in the hydrogen nucleus including proteum, deuterium or tritium and the binding energy according to equation (15).

The binding energy of a novel hydrino hydride ion can be expressed by the following equation.

(15)

(15)

에 의해 주어진 감소된 전자 질량이고, 여기서, mp는 양자의 질량이고, aH는 수소 원자의 반지름이며, a₀는 보어(Bohr) 반지름이고, e는 기본 전하이다. 상기 반지름들은 하기에 의해 주어진다. Here, p is an integer greater than 1, and s = 1/2, and π is pi, h is Planck's constant bar, μ ₀ is the vacuum permeability, m _e is the mass of the electron, μ _e is

, Where mp is the mass of both, aH is the radius of the hydrogen atom, a ₀ is the Bohr radius, and e is the base charge. These radii are given by

(16)

(16)

The binding energies of the hydrino hydride ions H ^- (n = 1 / p) as a function of p (where p is an integer) are shown in Table 1.

In accordance with the present invention, p = 2 to 23 in the case greater than the bond of the common hydride ion (about 0.8eV), p = 24 (H -) rather than a small, having a binding energy according to the formula (15-16) when A hydrinos hydride ion (H < ^- & gt ^; ) is provided. In the case of p = 2 to p = 24 in the formula (15-16), the binding energies of the hydride ions were 3, 6.6, 11.2, 16.7, 22.8, 29.3, 36.1, 42.8, 49.4, 55.5, 61.0, 65.6, 69.2, 71.6, 72.4, 71.6, 68.8, 64.0, 56.8, 47.1, 34.7, 19.3 and 0.69 eV. Also provided is a composition comprising the novel hydride ion.

The hydrino ion is distinguished from a common hydrogen ion and a common hydrogen ion containing two electrons having a binding energy of about 0.8 eV. The latter is referred to below as " normal hydrogen ion " or " normal hydrogen ion ". The hydrino hydride ion contains two indistinguishable electrons in the binding energy according to the formula (15-16) and the hydrogen nucleus comprising proteium, deuterium, or tritium.

There is provided a novel compound comprising at least one hydrinohydrate ion and at least one other element. The compound is referred to as a hydrino hydride compound.

Typical hydrogen species have the following bonding energies: (A) hydride ion, 0.754 eV ("normal hydride ion"); (b) hydrogen atom ("common hydrogen atom"), 13.6 eV; (c) a binary hydrogen molecule, 15.3 eV (" generic hydrogen molecule "); (d) hydrogen molecule ion, 16.3 eV (" generic hydrogen molecule ion "); And (e) H ⁺ ₃ , 22.6 eV (" having a common trihydrogen ". In this context, with respect to the hydrogen form, "normal" and "ordinary" to be.

(여기서, p는 정수로서, 바람직하게는 2 내지 137의 정수임)의 결합 에너지, 바람직하게는 ±10%, 보다 바람직하게는 ±5% 내의 결합 에너지를 갖는 수소 원자; (b) 약 According to another embodiment of the present invention, there is provided a pharmaceutical composition comprising (a)

(Where p is an integer, preferably an integer of 2 to 137), preferably a binding energy within ± 10%, more preferably ± 5%; (b) about

(여기서, P는 정수로서, 바람직하게는 2 내지 137의 정수임)의 결합 에너지, 바람직하게는 ±10%, 보다 바람직하게는 ±5% 내의 결합 에너지를 갖는 트리하이드리노(trihydrino) 분자 이온, H⁺ ₃(1/p); (e) 약

(여기서, P는 정수로서, 바람직하게는 2 내지 137의 정수임)의 결합 에너지, 바람직하게는 ±10%, 보다 바람직하게는 ±5% 내의 결합 에너지를 갖는 디하이드리노(diihydrino) 분자 이온; (f) 약

(여기서, P는 정수로서, 바람직하게는 2 내지 137의 정수임)의 결합 에너지, 바람직하게는 ±10%, 보다 바람직하게는 ±5% 내의 결합 에너지를 갖는 디하이드리노(diihydrino) 분자 이온과 같은 적어도 하나 의 결합 에너지가 증가된 수소종을 포함하는 화합물이 제공된다. Of the binding energy (where, p is an integer, preferably an integer of 2 to 24), preferably ± 10%, preferably a hydride ion having a binding energy within the ± 5% than the (H ^-); (c) H ⁺ ₄ (1 / p); (d) about

Trihydrino molecular ion having a binding energy of preferably within ± 10%, more preferably within ± 5%, of binding energy of H (where P is an integer, preferably an integer of 2 to 137), H ⁺ ₃ (1 / p); (e) about

A diihydrino molecular ion having a binding energy of preferably within ± 10%, more preferably within ± 5%, of a binding energy of an amino acid (wherein P is an integer, preferably an integer of 2 to 137); (f) about

Such as a diihydrino molecular ion having a binding energy within a binding energy of preferably 10% or more, more preferably +/- 5% There is provided a compound comprising at least one hydrogen species with increased binding energy.

According to another preferred embodiment of the present invention, (a)

(17)

(17)

 (Where p is an integer, h is a Planck constant, me is the mass of the electron, c is the flux in vacuum, μ is the mass of the reduced nucleus, k is the harmonic force constant (B) a total energy of preferably less than or equal to 10%, more preferably less than or equal to 5%, and (b)

(18)

(18)

At least one binding energy such as a dihydrino molecular ion having a total energy of at least 10%, preferably at least 10%, more preferably at least 5%, of the total energy of the total energy (where p is an integer and a ₀ is the bore radius) Lt; RTI ID = 0.0 > hydrogen < / RTI > species.

According to one embodiment of the present invention, where the compound comprises a hydrogen species with an increased binding energy that is negatively charged, the compound may be added with one or more cations such as protons, general H ⁺ ₂ , general H ⁺ ₃ .

(여기서, m은 1보다 큰 정수로서, 바람직하게는 400보다 작은 정수임)의 순 반응 엔탈피를 갖는 촉매와 반응시켜, 약

(여기서, p는 정수로서, 바람직하게는 2 내지 137의 정수임)의 결합 에너지를 갖는 결합 에너지가 증가된 수소 원자를 생성하는 단계를 포함한다.There is provided a method for preparing a compound comprising at least one or more hydride ions with increased binding energy. This compound is hereinafter referred to as a " hydrino hydride compound ". The method comprises dissolving a hydrogen atom at about

(Where m is an integer greater than 1, preferably less than 400)

(Where p is an integer, preferably an integer from 2 to 137) to produce a hydrogen atom with increased binding energy.

The additional product of the catalysis is energy. Hydrogen atoms with increased binding energy can react with electron sources to produce hydride ions with increased binding energy. The hydride ion having the increased binding energy may react with one or more cations to generate a compound containing hydride ions having an increased binding energy.

A composition of matter comprising a new type of hydrogen formed by the catalysis of new hydrogen species and atomic hydrogen is disclosed in " Mills Preceding Literature ". The hydrogen composition of the novel material comprises:

(a) at least one neutral, positive, or negative hydrogen species (hereinafter " hydrogen species with increased binding energy ") having the following bonding energies:

(i) binding energy greater than the binding energy of the corresponding common hydrogen species, or

(ii) Because the bond energy of a common hydrogen species is less than or equal to the thermal energy of ambient conditions (standard temperature and pressure, STP), the corresponding general hydrogen species is less stable than the binding energy of any hydrogen species that is unstable or unobserved. Greater binding energy; And

(b) at least one or more other elements. The compounds of the present invention are hereinafter referred to as " hydrogen bonds with increased binding energy ".

Here, " other element " means an element other than hydrogen species whose binding energy is increased. Thus, the other element may be any ordinary hydrogen species or any other element than hydrogen. In one group of compounds, hydrogen species with increased elemental and binding energies are neutral. In another group of compounds, hydrogen species with increased elemental and binding energies are charged so that the other element provides a balancing charge to form a neutral compound. The former group of compounds is characterized by molecular and coordination bonds; The latter group is characterized by ionic bonding.

Also provided are novel compounds and molecular ions comprising:

(a) at least one neutral, positive, or negative hydrogen species (hereinafter " hydrogen species with increased binding energy ") having the following total energy:

(i) a binding energy greater than the total energy of the corresponding generic hydrogen species, or

(ii) Because the total energy of a typical hydrogen species is less than or equal to the thermal energy of ambient conditions (standard temperature and pressure, STP), the corresponding general hydrogen species is less stable than the total energy of any hydrogen species that is unstable or unobserved. Greater total energy; And

(b) at least one other element.

The total energy of a hydrogen species is the sum of the energies for removing all electrons from the hydrogen species. The hydrogen species according to the present invention have a total energy greater than the total energy of the corresponding generic hydrogen species. Although some embodiments of hydrogen species with increased total energy may have a first electron binding energy that is less than the first electron binding energy of the corresponding common hydrogen species, the hydrogen species with increased total energy according to the present invention may also have a & Energy-enhanced hydrogen species ". For example, in the case of p = 24, the hydride ion of the formula (15-16) has a first binding energy lower than the first binding energy of the normal hydride ion, whereas when p = 24, 15-16) is much greater than the total energy of the corresponding normal hydride ion.

Also provided are novel compounds and molecular ions comprising:

(a) a plurality of neutral, positive, or negative hydrogen species (hereinafter " hydrogen species with increased binding energy ") having the following bonding energies,

(i) binding energy greater than the binding energy of the corresponding common hydrogen species, or

(ii) binding energy greater than the binding energy of any corresponding generic hydrogen species unstable or any unobservable hydrogen species, since the bond energy of a common hydrogen species is less than or equal to the thermal energy of the ambient conditions; And

(b) one optional element. The compounds of the present invention are hereinafter referred to as " hydrogen bonds with increased binding energy ".

A hydrogen species with an increased binding energy can be prepared by reacting one or more hydrino atoms with one or more electrons, a hydrino atom, a compound containing at least one hydrogen species with increased binding energy, and at least one other atom, Can be formed by reacting with an ion other than an increased hydrogen species.

Also provided are novel compounds and molecular ions comprising:

(a) a plurality of neutral, positive, or negative hydrogen species (hereinafter referred to as " hydrogen species with increased binding energy ") having the following total energy:

(i) a total energy greater than the total energy of a typical molecular hydrogen, or

(ii) the total energy of the corresponding generic hydrogen species is greater than the total energy of any hydrogen species that is unstable or unobservable, since the total energy of a common hydrogen species is less than or equal to the thermal energy of the ambient conditions; And

(b) one optional element. The compounds of the present invention are hereinafter referred to as " hydrogen bonds with increased binding energy ".

In one embodiment, (a) the binding energy according to equation (15-16) is greater than the binding energy (about 0.8 eV) of a general hydrogen ion and less than p = 24 for p = 2 to 23 (&Quot; hydride ion with increased binding energy " or " hydrinos hydride ion "); (b) a hydrogen atom (" hydrogen atom with increased binding energy " or " hydrinos ") having a binding energy greater than the binding energy of a common hydrogen atom (about 13.6 eV); (c) hydrogen molecules ("hydrogen molecules with increased binding energy" or "dihydrino") having a first binding energy greater than about 15.3 eV; And (d) at least one binding energy selected from the group consisting of molecular hydrogen ions ("molecular hydrogen ions with increased binding energy" or "dihydrolyn molecular ion") having binding energies greater than about 16.3 eV Lt; RTI ID = 0.0 > hydrogen < / RTI > species.

Characterization and identification of species with increased binding energy

New chemically generated or assisted plasma sources have emerged that can be a new source of power, based on resonant energy transfer mechanisms (rt-plasma) between hydrogen atoms and certain catalysts. The products are more stable hydrides and molecular hydrogen species such as H ^- (1/4) and H ₂ (1/4). The source operates by heating a hydrogen dissociator and a catalyst with an incandescent lamp to provide a hydrogen atom and a gaseous catalyst, respectively, and the catalyst reacts with hydrogen atoms to produce a plasma. (For example, 10 ³ K) from hydrogen atoms and specific atomizing elements or specific gas ions ionized singly or multiply at an integer multiple of 27.2 eV, which is the potential energy of a hydrogen atom, by Mills et al. [3-10] And extreme ultraviolet radiation (EUV) were observed at very low field strengths. Numerous independent experimental observations confirm that the rt plasma originates from the reaction of a novel hydrogen atom that produces hydrogen as a chemical intermediate in the quantum fraction state at a lower energy than the typical "bottom" (n = 1) state . The power is released [3, 9, 11-13] and the final reaction product is the new hydride compound [3, 14-16] or the low-energy molecular hydrogen [17]. Data supporting this include characteristic emissions from EUV spectroscopy [3-10, 13, 17-22, 25, 27-28], catalyst and hydride ion products [3, 5, 7, 21-22, 27-28] , Chemically formed plasma [3-10, 21-22, 27-28], considerable (> 100 eV) Ballmer alpha broadening [3-5, 7, 9-10, 12, 18-19, 21, 23-28], density reversal of H line [3, 21, 27-29], elevated electron temperature [19, 23-25], anomalous plasma afterglow afterglow [3, 8], power generation [3, 9, 11-13], and analysis of new compounds [3, 14-16].

Previously provided theories [6, 18-20, 30] are based on Maxwell's equation solving the structure of electrons. The familiar Reed-Berry equation (equation (19)) arises for the hydrogen-excited state of n> 1 in equation (20).

(19)

(19)

(20)

(20)

(p는 정수임) (21)An additional result is that the hydrogen atom undergoes a catalytic reaction with a particular atom, excimer, and ion that provides a reaction with a net enthalpy of the potential energy of the hydrogen atom, i.e., m · 27.2 eV (where m is an integer) It is possible. The reaction involves non-radioactive energy transfer, which forms a hydrogen atom, called hydrinos, which has a lower energy than the unreacted hydrogen atom corresponding to the fractional number of electrons. That is, in the case of the hydrogen-excited state,

(p is an integer) (21)

This replaces the well-known variable n = integer in the Reed-Berry equation. A hydrogen state with n = 1 and a hydrogen state with n = 1 / integer is non-radioactive but is capable of transitioning between two non-radioactive states, ie, n = 1 to n = 1/2, via non-radioactive energy transfer. Thus, the catalyst has a positive net reaction enthalpy of m · 27.2 eV (ie, it resonantly accepts non-radiative energy transfer from hydrogen atoms and releases energy to the periphery, affecting electron transfer to fractional quantum energy levels) to provide. As a result of the nonradiative energy transfer, the hydrogen atom becomes unstable and releases additional energy until it reaches a low energy nonradiative state with the main energy level given by Eqs. (19) and (21). Processes that occur without photons and require collisions, such as hydrogen bonding, are common [31]. In addition, some commercially available phosphors are based on resonant non-radiative energy transfer involving multipole coupling.

Two H (1 / p) react to form H ₂ (1 / p). Hydrogen molecule ion and molecular charge and current density action, bond distance, and energy have traditionally been solved with surprising accuracy [30, 33]. Using Laplacian in an ellipsoidal coordinate with a non-radiative constraint, the central field of the + pe at each focus of the prolate spheroid molecular orbital The total energy of the hydrogen molecule is:

                                                                   (22)

Where p is an integer, h is a Planck constant, m _e is the mass of the electron, C is the flux in vacuum, μ is the mass of the reduced nucleus, k is the base constant [30, 33] , And a ₀ is the radius of the bore). The vibration and rotational energy of fraction-lead beryl-state molecular hydrogen H ₂ (1 / p) is P ² times H ₂ . Thus, in the case of the transition of the hydrogen-form molecule H ₂ (1 / p) from v = 0 to v = 1, the vibration energy Evib

Evib = P20.515902 eV (23)

EH ₂ (υ = 0 → υ = 1), which is the experimental vibration energy when H ₂ transitions from υ = 0 to υ = 1, is described by Beutler [34] and Herzberg [35 ]). The rotational energy when the hydrogen-form molecule H ₂ (1 / p) transitions from J to J + 1, Erot [30, 33]

(24)

(24)

(Where I is the moment of inertia and the experimental rotational energy when H ₂ transitions from J = 0 to J = 1 is given by Atkins [36]). The p ² dependence of the rotational energy results from the inverse p dependence of the inter-nucel distance and the impact on the corresponding I. The predicted internuclear distance 2c 'of H ₂ (1 / p) is:

(25)

(25)

The rotational energy allows a very accurate measurement of I and inter-nucetal distances using well-established theories [37].
Ar ⁺ can function as a catalyst because the ionization energy is about 27.2 eV. In Ar ⁺ catalyst reaction to Ar ²⁺ forms a H (1/2), which in addition functions as a catalyst and a reaction to form an H (1/4) [19-20, 30 ]. Therefore, H (1/4) is expected to be observed in dependence on the flow, because it requires the accumulation of an intermediate in the formation of H ₂ (1/4). The mechanism was tested by an experiment using a flowing plasma gas. In the case of a high pressure argon-hydrogen plasma excited by a 12.5 keV electron beam, neutral molecular emission was expected. For H ₂ (1/4), a spinning line was expected and was found in the 150-250 nm region. The spectral lines were compared with those predicted by the equation (23-24) corresponding to the inter-nucleus distance of 1/4 of H ₂ given by equation (25). For p = 4 in Eqs. (23-24), the predicted energies for a series of υ = 1 → υ = 0 oscillation-rotation of H ₂ (1/4) are as follows:

delete

(26)

(26)

Since He ⁺ ionizes at 54.417 eV, which is 2 · 2.27 eV, it also meets catalytic conditions that the change in enthalpy of the chemical or physical process must be the same as an integral multiple of 27.2 eV. The product H (1/3) of the catalytic reaction of He ⁺ can additionally act as a catalyst to form H (1/4) and H (1/2) [19-20, 30] Can induce a transition to H (1 / p). q 13.6 eV, where q = 1, 2, 3, 4, 6, 7, 8, or 11, is irradiated with ultraviolet radiation recorded at microwave discharge with 2% hydrogen of helium (EUV) spectroscopy [18-20]. The lines corresponded to H (1 / p), which is the fractional Reid Berry state of the hydrogen atom given by Eqs. (19) and (21).

Rotating lines were observed in the region of 145-300 nm from an argon - hydrogen plasma excited by an atmospheric electron beam. The energy gap of 4 ² times of the unprecedented hydrogen was confirmed to be 1/4 times of H ₂ and H ₂ (1/4) (Equation (23-26)). The H ₂ (1 / p) gas was separated by liquefying the helium-hydrogen plasma gas using a liquid nitrogen cold trap capable of high-vacuum (10 ^-6 Torr) and was separated by mass spectroscopy Respectively. The condensable gas has a higher ionization energy than H ₂ by MS [17]. Catalysis - H ₂ (1/4) gas obtained from the lysis of the plasma gas as well as from the chemical decomposition of the hydride containing the corresponding hydride ion H ^- (1/4) has a H ₂ of 4.63 The upfield was identified as a shifted single peak at 2.18 ppm versus the identified. (FTIR) spectroscopy of solid samples containing H ^- (1/4) from an electron beam with an argon - hydrogen plasma maintained and interstitial H ₂ (1/4) H ₂ (1/4) has been further identified by a study of H ₂ .

Using the calorimetry of the reservoir, it was determined whether a measurable power in the rt plasma occurred due to the reaction forming the state given by Eqs. (19) and (21). Specifically, He / H ₂ (10%) (500 mTorr), Ar / H ₂ (10%) (500 mTorr) and H ₂ O (g) produced using an Evenson microwave cavity, (500 and 200 mTorr) plasma produced 5% higher heat than non-rt-plasma such as He, Kr, Kr / H ₂ (10%) under the same conditions as gas flow, pressure and microwave operating conditions. The excess power density of the rt-plasma was about 10 W · cm-3. In addition to the unique Vacuum Ultraviolet (VUV), earlier studies on this rt-plasma have shown a sharp increase in line width of the hydrogen-based halogen line [3-5, 7, 9-10, 12, 18-19, 21, 23-28] , There are other unique characteristics including the density reversal of the hydrogen-excited state. Present and past results are consistent with the existence of an unknown pyrogenic reaction occurring in the rt-plasma.

Since the ionization energy from Sr + to Sr 3+ has a net reaction enthalpy of 2 · 27.2 eV, Sr + can function alone or as a catalyst with an Ar + catalyst. It has been previously reported that the rt plasma is formed with a low field (1 V / cm) at a low temperature (e.g., 103 K) from strontium evaporated by heating and hydrogen atoms generated in the tungsten filament [4-5,7,9-10]. Increased with the addition of argon, strong VUV emissions were observed, but did not increase when sodium, magnesium or barium replaced strontium or hydrogen, argon or strontium alone. Characteristic emissions were observed from the continuum state of Ar2 + at 45.6 nm, without the typical Reidberg series Ar I and Ar II lines, confirming that 27.2 eV of resonance-nonradiative energy was transferred from the hydrogen atom to Ar +. Predicted Sr3 + emission lines were also observed from the strontium-hydrogen plasma supporting the rt-plasma mechanism [5, 7]. A time-dependent linewidth increase of the H-Ballmer? Line corresponding to very fast H (25 eV) was observed. An excess power of 20 mW · cm- was calorimetrically determined on the rt-plasma formed when Ar + was added to Sr + as an addition catalyst.

와 비교하였다. 동일한 광출력을 얻기 위하여, 수소-나트륨, 수소-마그네슘, 및 수소-바륨 혼합물은 수소-스트론튬 혼합물의 전력의 각각 4000, 7000, 및 6500 배를 요구하였고, 아르곤의 첨가시 약 2배 만큼 상기 비율이 증가하였다. 수소-스트론튬 혼합물의 경우, 수소 단독 및 나트륨-수소 혼합물의 경우가 250 V, 수소-마그네슘 및 수소-바륨 혼합물의 경우가 약 140-150 V와 비교하여 볼 때, 약 2 V의 매우 낮은 전압에서 글로 방전(glow discharge) 플라즈마를 형성하였다 [4-5, 7]. 이러한 전압은 너무 낮아서 적용 장(field)이 높은 가속화 이온을 포함하는 통상적인 메커니즘에는 적용할 수 없다. 낮은 전압의 EUV 및 가시광선 공급원이 유용하다[10]. Significant linewidth enhancement of the Ballmer a line, corresponding to an average hydrogen atom temperature of 14, 24 eV, and 23-45 eV, was observed for strontium and argon-strontium rt-plasmas, and strontium-hydrogen, helium- Strontium-helium-hydrogen, and strontium-argon-hydrogen, respectively, for pure hydrogen, xenon-hydrogen, and magnesium-

. To obtain the same light output, the hydrogen-sodium, hydrogen-magnesium, and hydrogen-barium mixtures required 4000, 7000, and 6500 times of the power of the hydrogen-strontium mixture, respectively, Respectively. In the case of a hydrogen-strontium mixture, the hydrogen alone and in the case of the sodium-hydrogen mixture in the case of 250 V, the hydrogen-magnesium and the hydrogen-barium mixture in the case of the very low voltage of about 2 V To form a glow discharge plasma [4-5, 7]. This voltage is too low to be applicable to conventional mechanisms involving high acceleration fields. Low voltage EUV and visible light sources are useful [10].

의 반지름까지 m 준위 이하로 떨어진다. K가 K3+로 되면서 수소 원자의 포텐셜 에너지의 3배, 즉 3·27.2 eV만큼의 순 엔탈피를 갖는 반응을 제공하기 때문에, K는 촉매로 기능하여 촉매작용을 겪는 각 일반적인 수소 원자들이 총 204 eV를 방출하게 할 수 있다[3]. 그리고 나서, K는 생성물인 H(1/4)과 반응하여 낮은 상태의 H(1/7)을 형성하거나, 불균형이라 불리는 공정에서 하이드리노만을 포함하는 다음과 같은 추가적인 촉매 전이가 일어날 수 있다:

등. 포텐셜 에너지의 다극 확대(multipole expansion)에 대응하는 하이드리노의 이온화 에너지 및 준안정 공진 상태(metastable resonant state)가 이전에 주어진 바와 같이[19-20, 30], m·27.2 eV (수식 (10 및 (21))이기 때문에, 촉매작용이 시작되면 하이드리노는 추가로 더 낮은 상태로의 전이를 자가촉매한다. 이 메커니즘은 무기 이온 촉매작용의 메커니즘과 유사하다. 제1 하이드리노 원자로부터 제2 하이드리노 원자로 m·27.2 eV의 에너지가 전달되면 제1 원자의 중심장이 m 배만큼 증가하고 전자가 반지름

에서 반지름

로 m 준위 아래로 떨어진다. 촉매 생성물 H(1/p)는 또한 전자와 반응하여 다음의 결합 에너지 EB를 갖는 신규 수소화물 이온 H^-(1/p)을 형성할 수 있다[3, 14, 16, 21, 30] In general, when an energy of m · 27.2 eV is transferred from a hydrogen atom to a catalyst, the center field interaction of H atoms increases by m times, and electrons increase from a hydrogen atom radius aH

To the radius of m. Since K provides a reaction with a net enthalpy of 3 · 27.2 eV, which is three times the potential energy of a hydrogen atom, as K 3 +, K functions as a catalyst so that each typical hydrogen atom undergoing catalysis has a total of 204 eV Can be released [3]. Then K reacts with the product H (1/4) to form a low state H (1/7), or in the process called imbalance, the following additional catalytic transition involving hydrinos may occur:

Etc. The ionization energy and metastable resonant state of the hydrino corresponding to the multipole expansion of the potential energy are given as [19-20, 30], m 占 27.2 eV (Equations (10) and (21), the initiation of the catalytic action causes the hydrinos to autocatalyst to an additional lower state. This mechanism is analogous to the mechanism of inorganic ion catalysis. From the first hydrino atom to the second hydride atom When the energy of the Reno atom m · 27.2 eV is transferred, the center length of the first atom is increased by m times and the electron is radiated

Radius at

M falls below the m-level. The catalytic product H (1 / p) can also react with electrons to form a new hydride ion H ^- (1 / p) with the following binding energy EB [3, 14, 16, 21, 30]

(27)

(27)

(여기서, mp는 양자의 질량이고, aH는 수소 원자의 반지름이며, a0는 보어 반지름이고, e는 기본 전하임)에서 주어진 감소된 전자 질량임). 이온 반지름은

이다. 수식 (27)로부터, 계산된 수소화물 이온의 이온화 에너지는 0.75418 eV이고, 리케(Lykke)[38]에 의한 실험값은 6082.99±0.15 cm-1(0.75418 eV)이다. (Where p is an integer greater than 1, S = 1/2, h is Planck's constant, mu is vacuum permeability, me is an electronic mass,

(Where mp is the mass of both, aH is the radius of the hydrogen atom, a0 is the radius of the bore, and e is the reduced electron mass given by the basic charge). The ion radius

to be. From equation (27), the calculated ionization energy of the hydride ion is 0.75418 eV and the experimental value by Lykke [38] is 6082.99 ± 0.15 cm-1 (0.75418 eV).

The actual evidence of an active catalytic reaction, including the resonant energy transfer between a hydrogen atom and K forming a highly stable new hydride ion H ^- (1 / p), called the hydrinos hydride with a predicted fractional number p = 4 Have been previously reported [3]. Characteristic emissions were observed from K3 +, confirming the transfer of resonant non-radiative energy of 3 · 27.2 eV from hydrogen atom to K. From equation (27), the binding energy EB of H ^- (1/4) is as follows:

 EB = 11.232 eV (? Vac = 1103.8 Å) (28)

The product hydride ion H ^- (1/4) was spectroscopically observed at 110 nm corresponding to the predicted binding energy of 11.2 eV [3, 21].

는 H^-(1/1)의 시프트 및 낮은 전자 에너지 상태로 인한 공헌도의 합으로 주어진다:The upfield-shifted NMR peak is a direct evidence that there is a low-energy state of hydrogen with a reduced radius compared to normal hydride ions, with increased diamagnetic shielding of both. The total theoretical shift for H ^- (1 / p)

Is given as the sum of the contribution due to the shift of H ^- (1/1) and the low electron energy state:

(29)

(29)

(Where p = integer > 1). The corresponding alkali hydrides and alkaline hydrino hydrides (including H ^- (1 / p)) were identified by 1H MAS NMR and compared with theoretical values. The agreement between the predicted peak and the observed peak indicates the accuracy of the test.

The 1H MAS NMR spectrum of the novel compound KH * Cl versus the external tetramethylsilane (TMS) showed a large and clear upfield resonance at -4.4 ppm, corresponding to an absolute resonance shift of -35.9 ppm, [3, 14-16]. These results show that the strong hydrogen Lyman-emitting rt-plasma, the fixed inverted Lehman density, the afterglow duration, the highly active hydrogen atom, the characteristic alkali-ion release due to catalysis, Previous observations from new spectral lines, and measurements of power beyond conventional chemistry [3], have confirmed the catalytic reaction of atomic hydrogen to form more stable hydride ions named H ^- (1 / p) Consistent with the forecast. Since comparison of the theoretical and experimental shifts of KH * Cl is a direct proof of low-energy hydrogen with strong intrinsic intrinsic onset, additional analysis by infrared (FTIR) spectroscopy to remove any known explanation [39] .

As a result of the basic analysis [14, 16], these compounds were found to contain alkali metals, halogens and hydrogen, and known hydride compounds with up field-shift hydride NMR peaks in this composition were not found in the literature. Typical alkali hydrides mixed with or alone in alkaline hydrides indicate down-field shift peaks [3, 14-16]. In the literature, it is limited to U centered H that can be used as an alternative to H ^- (1 / p) as a possible source of upfield NMR peaks. A strong and distinctive infrared rotation band at 503 cm-1 produced by the replacement of Cl- with H ^- in KCl allowed removal of the U center H as a source of upfield-shift NMR peaks [39].

As a further identification, the X-ray photoelectron spectrum (XPS) of the hydrino hydride KH * I was performed to determine if the predicted H ^- (1/4) binding energy given by equation (28) , FTIR analysis of the crystals with H <"& gt ^; (1/4) before and after storage in argon for 90 days is performed to determine the interstitial H ₂ (1 / 4) were searched. Identifying a single rotation peak in an energy state with ortho-para splitting due to the free rotation of a very small hydrogen molecule would be a valid proof of existence because there are no other potential challenges [39].

Rotating the release of H ₂ (1/4) is H ^- were observed in the (1/4) the determination of KH * I having a peak of the vibration of H ₂ (1/4) - rotation release H ₂ (1 / 4) where impact (excitation) as was observed from 12.5 keV- electron beam maintain an argon plasma having a 1% hydrogen in, the H ₂ (1/4) trapped in the lattices of KH * Cl, or H in the ^- (1/4 (1/4) or H ₂ (1/4) formed in situ from the K catalysis of H through the bombardment formed H ₂ (1/4) formed from gas , A windowless EUV spectrometer on the electron beam excitation of the crystal using a 12.5 keV electron gun. The rotational energy of H ₂ (1/4) was also confirmed by the above technique. Consistent results from extensive investigative techniques provide clear evidence that hydrogen can be present in low energy states in the form of H ^- (1/4) and H ₂ (1/4), previously thought to be possible. In one embodiment, the products of the Li and NaH catalytic reactions are H ^- (1/4) and H ₂ (1/4), and in the case of NaH additionally H ^- (1/3) and H ₂ )to be. The present invention is based on their identification and their characteristic emission from EUV spectroscopy, catalyst and hydride ion products, low energy hydrogen emission, chemically formed plasma, unique Ballmer alpha linewidth increase, H line density inversion, elevated electron temperature, sustained afterglow, power generation, and analysis of new compounds to provide the corresponding active exothermic response. Species H ^- (1 / p) and H ₂ (1 / p) A preferred check technique is H in ^- (1 / p) and H ₂ (1 / p) of NMR, crystals within the captured H ₂ (1 / p) of ^{FTIR, H - (1 / p} ) of the ^{XPS, H - (1 / p} ) of the _{TOF-SIMS, H 2 (1} / p) electron beam here emission spectroscopy, the H ₂ (1 / p) trapped within the crystal lattice of of the electron beam emission spectroscopy, and H ^- (1 / p) is the TOF-SIMS identification of novel compounds, including. Preferred techniques for vigorous catalysis and power balance are line broadening, plasma formation, and calorimetry. Preferably, H ^- (1 / p) and H ₂ (1 / p) are H ^- (1/4) and H ₂ (1/4), respectively.

Brief Description of Drawings

1A is a schematic diagram of an energy reactor and a power plant according to the present invention.

2A is a schematic diagram of an energy reactor and a power generation apparatus for recycling or regenerating fuel according to the present invention.

3A is a schematic diagram of a power reactor according to the present invention.

4A is a schematic diagram of discharge power and plasma cell and reactor according to the present invention.

BRIEF DESCRIPTION OF THE DRAWINGS Figure 1 is an experimental apparatus comprising a filament gas cell forming a lithium-argon-hydrogen and lithium-hydrogen rt-plasma.

Figure 2 is a schematic of the reaction cell used to measure the energy balance of the NaH catalytic reaction to form the hydrinos and a cut plane of the water flow calorimetry. The configuration is as follows: 1-in / out thermistor; 2-high temperature valve; 3-ceramic fiber heater; 4-copper water cooling coil; A 5-reactor; 6-insulator; 7-cell thermocouple, and 8-flow chamber.

3 is a schematic view of a flow calorimeter used to measure the energy balance of the NaH catalytic reaction forming the hydrinos.

4 is a reaction mixture (i) R-Ni, Li , LiNH 2, and LiBr or LiI or (ii) Pt / Ti dissociation claim, Na, NaH, and the reactants and LiH containing as NaCl or NaBr * Br, LiH * I, NaH * Cl, and NaH * Br. The configuration is as follows: 101-stainless steel cell; 117-inner cavity of the cell; 118 - High vacuum con- fllat flange; 119-mating blank cone flange; 102-Stainless Steel Tube Vacuum Lines and Gas Supply Lines; 103-kiln or top insulator lid, 104-heater cover wrapped in high temperature insulator; 108-Pt / Ti dissociation agent; 109-reactant; 110-High vacuum turbo pump; 112-Pressure gauge; 111-Vacuum pump valve; 113-valve; 114-valve; 115-regulating device, and 116-hydrogen tank

Figure 5 shows the 656.3 nm Ballmer alpha linewidth recorded with a high resolution visual spectrometer at (A) at the initial discharge of the lithium-argon-hydrogen rt-plasma and (B) at 70 hours of operation. Significant broadening of the lithium line and unique H line was observed for a time corresponding to an average hydrogen atom temperature of > 40 eV and a fractional density of greater than 90%.

Figure 6 shows a 656.3 nm Ballmer alpha linewidth recorded with a high resolution (+/- 0.006 nm) time spectrometer at (A) at the initial discharge of the lithium-hydrogen-plasma and (B) at 70 hours of operation. Lithium lines and unique H line broadening were observed over time, but decreased compared to those with argon - hydrogen evolution (95/5%).

Figure 7 shows DSC (100-750 ° C) results for NaH at a scan rate of 0.1 degrees / minute. A broad exotherm peak was observed at 350-420 ° C., corresponding to 47 KJ / mole, consistent with sodium hydride decomposition at this temperature range with a corresponding enthalpy of 57 KJ / mole. Was a large exothermic observed under the conditions applied to form the catalyst NaH in the region of 640 to 825 ℃, which, if the H largest exothermic reaction in the hydrogen combustion enthalpy, that is, -241.8 KJ / mole H ₂ is greater than at least -354 KJ / mole H ₂ .

Figure 8 shows the results of DSC (100-750 ° C) of MgH ₂ at a scanning rate of 0.1 degrees / minute. Two sharp endothermic peaks were observed. The first peak centered at 351.75 ° C, corresponding to 68.81 KJ / mole MgH ₂ , corresponds to a decomposition energy of 74.4 KJ / mole MgH ₂ . The second peak at 647.66 ° C, corresponding to 6.65 KJ / mole MgH ₂ , corresponds to a known melting point of Mg (m) of 650 ° C and a fusion enthalpy of 8.48 KJ / mole MgH ₂ . Therefore, the predicted behavior was observed in the case of decomposition of the non-catalytic hydrides in the control group.

Figure 9 shows temperature versus time for a calibration run with a vacuum test cell and a resistive heating device.

Figure 10 shows power versus time for a calibration run with a vacuum test cell and a resistive heating device. The numerical integration of the input and output power curves represents an output energy of 292.2 KJ and an input energy of 303.1 KJ, corresponding to a combined output cooling of 96.4% of the resistive input.

Figure 11 shows the cell temperature over time for a cell containing a reagent comprising a catalytic material, 1 g Li, 0.5 g LiNH ₂ , 10 g LiBr, and 15 g Pd / Al ₂ O 3 and a hydrinot reaction. The reaction did not reach 120 seconds, resulting in 19.1 KJ of energy, resulting in a system-response-corrected peak power of greater than 160 W.

12 shows the catalyst material, 1 g Li, 0.5 g LiNH 2, 10 g LiBr, and 15 g Pd / Al ₂ O ₃ in accordance with the cooling power during the time selwa hydroxy Reno reaction containing reagents comprising a. The numerical integration of the input and output power curves with the applied calibration correction produced an output energy of 227.2 kJ corresponding to an excess energy of 19.1 kJ and an input energy of 208.1 kJ.

Figure 13 shows the cell temperature over time for a cell containing a reagent comprising R-Ni, 15 g R-Ni / Alalloy powder as starting material, and 3.28 g Na and R-Ni control power test.

Figure 14 shows the cooling power over time for a control power test with a cell containing a reagent comprising R-Ni, 15 g R-Ni / Alalloy powder as starting material, and 3.28 g Na. The energy balance was obtained by a calibration-calibrated numerical integration of the input and output power curves producing an output energy of 384 kJ and an input energy of 385 kJ.

Figure 15 shows the cell temperature over time in a cell containing a reagent comprising a catalytic material, 15 g NaOH-doped R-Ni 2800, and 3.28 g of Na and a hydrinot reaction. The reaction took less than 90 seconds to release 36 KJ of energy, resulting in a system-response-corrected peak power of greater than 0.5 W.

Figure 16 shows the cooling power over time for a cell containing a catalyst material, a reagent comprising 15 g NaOH-doped R-Ni 2800, and 3.28 g Na and a hydrinoc reaction. The numerical integration of the input and output power curves with the applied calibration calibration produced an output energy of 185.1 kJ corresponding to an excess energy of 36 kJ and an input energy of 149.1 kJ.

Figure 17 shows the temperature of the cell over time in the presence of the catalyst material, the reagent containing 15 g NaOH-doped R-Ni 2400 and the hydrinos. The cell temperature jumped from 60 ° C to 205 ° C in 60 seconds and the reaction emitted 11.7 KJ of energy in a short time resulting in a system-response-corrected peak power exceeding 0.25 W.

Figure 18 shows the cooling power over time for a cell containing a reagent comprising a catalytic material, 15 g NaOH-Doped R-Ni 2400 and a hydrinos reaction. The numerical integration of the input and output power curves with the calibration correction produced an input energy of 184.0 kJ corresponding to an output energy of 195.7 kJ and an excess energy of 11.7 kJ.

Figure 19 shows the positive TOF-SIMS spectrum of LiBr (m / e = 0-100).

Figure 20 shows the positive TOF-SIMS spectrum (m / e = 0-100) of LiH * Br crystals.

Figure 21 shows the negative TOF-SIMS spectrum of LiBr (m / e = 0-100).

Figure 22 shows the negative TOF-SIMS spectrum (m / e = 0-100) of a LiH * Br crystal. The major hydrides, LiHBr ^- , and Li ₂ H ₂ Br ^- peaks were uniquely observed.

Figure 23 shows the positive TOF-SIMS spectrum of LiI (m / e = 0-200).

24 shows the positive TOF-SIMS spectrum (m / e = 0-200) of LiH * I crystals. LiH ⁺ , Li ₂ H ₂ I ⁺ , Li ₄ H ₂ I ⁺ , and Li ₆ H ₂ I ⁺ were observed only in the cation spectrum of LiH * I crystals.

Figure 25 shows the negative TOF-SIMS spectrum of LiI (m / e = 0-180).

26 shows the negative TOF-SIMS spectrum (m / e = 0-180) of the LiH * I crystal. The major hydrates, LiHI ^- , Li ₂ H ₂ I ^-, and NaHI ^- were uniquely observed.

Figure 27 shows the negative TOF-SIMS spectrum (m / e = 20-30) of NaH * -coated Pt / Ti with the generation of excess heat of 15 kJ. The hydrinos hydride compound NaHx <"> ^- was observed.

28 shows a positive TOF-SIMS spectrum (m / e = 0-100) of R-Ni reacted at 50 ° C for at least 48 hours. The major ion on the surface was Na ^+, which is consistent with NaOH doping on the surface. In addition, other principal element ions of R-Ni 2400 such as Al ⁺ , Ni ⁺ , Cr ⁺ , and Fe ⁺ were observed.

29 shows a negative TOF-SIMS spectrum (m / e = 0-180) of R-Ni reacted at 50 ° C for 48 hours or more. Sodium hydrinos hydride and NaH ^- and NaH ₃ NaOH ^- which are the main hydrides to which NaOH is bonded, as well as sodium hydrinos hydride NaH _x ^- bonded to NaOH, NaO, OH and O ^- Unique ions were observed.

Figures 30A-B show 1H MAS NMR spectra versus external TMS.

(A) LiH * Br represents a broad -2.5 ppm upfield-shift peak corresponding to H ^- (1/4) and H ₂ (1/4), respectively, and a peak at 1.13 ppm,

(B) LiH * I are each ^H-peak at 1.06 ppm and 4.38 ppm corresponding to the peak shift, and H ₂ (1/4), and H ₂ - (1/4) corresponding to a wide field-up -2.09 pppm .

Figures 31A-B show 1H MAS NMR spectra versus external TMS.

(A) KH * Cl represents a very sharp -4.46 ppm up field-shift peak corresponding essentially to the free ion environment,

(B) KH * I represents a -2.31 ppm up field-shift peak similar to that of LiH * Br and LiH * I. Both spectra also had a 1.13 ppm peak corresponding to H ₂ (1/4).

Figures 32A-B are graphs showing the H content selectivity of LiH * X versus molecular species, based on the non ^- polarity of the halide and the corresponding non-reactivity to H- (1/4) MAS NMR spectrum. (A) LiH * F is a peak (H at 1.16 ppm corresponding to the peak, and H ₂ (1/4) at 4.31 ppm for the H ₂ containing non-fluorine-polarization ^(1/4) ion peak that represents a no), including (B) a non-polarized chlorine Cl * is LiH peak at 1.2 ppm corresponding to the peak, and H ₂ (1/4) at 4.28 ppm corresponding to H ₂ (H ^- (1 / 4) no ion peak).

H 33 is ^respectively external showing the peak of the peak shift, the peak at 1.13 ppm, and 4.3 ppm - (1/4), H 2 (1/4), and -3.58 ppm up field corresponding to the H ₂ The 1H MAS NMR spectrum of NaH * Br versus TMS is shown.

Figure 34A-B is _{H 2, H 2 (1/4)} , and H ^- shows the effect of hydrogen addition on the relative strength of (1/4). Hydrogenation increased the H ^- (1/4) peak and H ₂ (1/4) while H ₂ increased. (A) NaH * Cl synthesized by hydrogenation corresponds to -4 ppm upfield shift peak corresponding to H ^- (1/4), 1.1 ppm peak corresponding to H ₂ (1/4), and H ₂ (B) NaH * Cl synthesized without hydrogenation shows a main peak of 4 ppm corresponding to H ^- (1/4), a main peak corresponding to H ₂ (1/4) 1.0 ppm peak, and a small 4.1 ppm peak corresponding to H ₂ .

35 is NaCl and represents the only hydrogen supplied causes the solid acid external TMS contrast 1H MAS NMR spectrum of a NaH Cl * produced from the reaction of KHSO _4, NaH wherein * is H, Cl at -3.97 ppm ^- (1/4) peak and Shift peak at -3.15 ppm corresponding to H ^- (1/3). The peaks corresponding to H ₂ (1/4) and H ₂ (1/3) appear at 1.15 ppm and 1.7 ppm, respectively. The positive fraction was hydrogen conditions exist, since the synthesis NaH * Cl using a solid acid as a source of H without addition of hydrogen gas and the dissociation (dissociator), H ₂ was not a peak exists at 4.3 ppm. (SB = side band).

Figures 36A-B show XPS emission spectra (E _b = 0 eV to 1200 eV). (A) LiBr. (B) LiH * Br.

Figure 37 shows the 0-85 eV binding energy region of the high resolution XPS spectrum of LiH * Br and control LiBr (dashed). The XPS spectrum of LiH * Br differs from LiBr in that it has additional peaks at 9.5 eV and 12.3 eV, which do not correspond to known elements or peaks of other major elements. The peaks correspond to H ^- (1/4) in two different chemical environments.

Figures 38A-B show XPS emission spectra (E _b = 0 eV to 1200 eV). (A) NaBr. (B) NaH * Br.

Figure 39 shows the 0-40 eV binding energy region of the high resolution XPS spectrum of NaH * Br and control NaBr (dashed). The XPS spectrum of NaH * Br differs from that of NaBr in that it has additional peaks at 9.5 eV and 12.3 eV, which do not correspond to known elements or peaks of other major elements. The peaks correspond to H ^- (1/4) in two different chemical environments.

Figures 40A-B show XPS emission spectra (E _b = 0 eV to 1200 eV). (A) Pt / Ti. (B) NaH * -coated Pt / Ti with the generation of 15 kJ of excess heat.

Figures 41A-B show high resolution XPS spectra (E _b = 0 eV to 100 eV). (A) Pt / Ti. (B) NaH * -coated Pt / Ti with the generation of 15 kJ of excess heat. The Pt4f _7/2 , Pt4f _5/2 , and O2s peaks on NaH * -coated Pt / Ti were observed at 70.7 eV, 74 eV, and 23 eV, respectively, and for Pt / Ti the outermost valence band was unique Respectively. The Na 2p and Na 2s peaks were observed at 31 eV and 64 eV on NaH * -coated Pt / Ti, and the outermost bands were observed only for Pt / Ti.

Figures 42A-B show high resolution XPS spectra (E _b = 0 eV to 50 eV). (A) Pt / Ti. (B) NaH * -coated Pt / Ti with the generation of 15 kJ of excess heat. The XPS spectrum of NaH * -coated Pt / Ti differs from that of Pt / Ti in that it has additional peaks at 6 eV, 10.8 eV, and 12.8 eV, which do not correspond to known elements or other key element peaks. The 10.8 eV and 12.8 eV peaks correspond to H ^- (1/4) in two different chemical environments, and the 6 eV peak corresponds to H ^- (1/3). Thus, the fractional hydrogen state, 1/3 and 1/4, existed as predicted by equation (27).

43 shows the XPS irradiation spectrum (E _b = 0 eV to 120 eV) of NaH * -coated Si whose main element peaks were confirmed.

Figure 44 shows the XPS emission spectra (E _b = 0 eV to 120 eV) of NaH * -coated Si with peaks at 6 eV, 10.8 eV and 12.8 eV, corresponding to known elements or other key element peaks . The 10.8 eV and 12.8 eV peaks corresponded to H ^- (1/4) in two different chemical environments, and the 6 eV peak corresponded to H ^- (1/3). Thus, the fractional hydrogen states, 1/3 and 1/4, were consistent with the results of the NaH * -coated Pt / Ti shown in Figure 42B as predicted by equation (27).

Figures 45A-B show high resolution (0.5 cm ^-1 ) FTIR spectra (490-4000 cm ^-1 ). (A) LiBr. (B) LiH * Br with an NMR peak corresponding to H ^- (1/4) heated to > 600 ° C under dynamic vacuum maintained at -2.5 ppm NMR peak. The amide peaks at 3314, 3259, 2079 (broad), 1567, and 1541 cm ^-1 and the imide peaks at 3172 (broad), 1953, and 1578 cm ^-1 were removed; Thus, they were not the source of the maintained -2.5 ppm NMR peak. The -2.5 ppm in the 1H MAS NMR spectrum corresponds to H ^- (1/4). Further, the FTIR peak at 1989 cm ^-1 could not correspond to any known compound but was consistent with the predicted frequency of para H ₂ (1/4).

Figure 46 shows a 150-350 nm spectrum of electron beam excited CsCl containing H ₂ (1/4). A series of flattened lines were observed in the 220-300 nm region, consistent with the spacing and strength profile of the P branch of H ₂ (1/4).

Figure 47 shows a spectrum of 100-550 nm of an electron beam excited silicon wafer coated with NaH * Cl containing H ₂ (1/4). A series of flattened lines were observed in the 220-300 nm region, consistent with the spacing and strength profile of the P branch of H ₂ (1/4).

DETAILED DESCRIPTION OF THE PREFERRED EMBODIMENTS

Hydrogen catalytic reactor

A hydrogen catalytic reactor 50 for producing energy and low energy hydrogen species in accordance with the present invention is shown in Figure 1A and includes an energy reaction mixture 54, a heat exchanger 60, and a steam generator 62 and a turbine 70, And a vessel 52 containing a power converter, such as a power converter. In one embodiment, the catalysis includes reacting hydrogen atoms from the source 56 with the catalyst 58 to form a low energy hydrogen " hydrinos " and generate power. The heat exchanger 60 absorbs the heat released by the catalytic action when the reaction mixture composed of hydrogen and the catalyst reacts to form low energy hydrogen. The heat exchanger exchanges heat with a steam generator (62) that absorbs heat from the exchanger (60) and generates steam. The energy reactor 50 further includes a turbine that receives steam from the steam generator 62 and then supplies mechanical power to a power generator 80 that converts steam energy to electrical energy, The energy is transferred to the rod 90 for producing or dissolving the work.

In one embodiment, the energy reaction mixture 54 comprises an energy-emitting material 56, such as a solid fuel, supplied via a supply passage 42. Wherein the reaction mixture comprises a source of a source of hydrogen isotope atoms, a source of molecular hydrogen isotopes, and a source of a catalyst (58) that resonantly removes about 27.2 eV to form low-energy hydrogen atoms, wherein m is Is an integer, preferably an integer less than 400, and the reaction with hydrogen in the low energy state occurs by contacting hydrogen with the catalyst. The catalyst may be molten, liquid, gaseous or solid. The catalytic action releases energy in the form of heat and forms at least one of low-energy hydrogen isotope atoms, molecules, hydride ions, and low-energy hydrogen compounds. Thus, the power cell also includes a low-energy hydrogen chemical reactor.

The hydrogen source may be hydrogen gas, dissociation of water including thermal dissociation, electrolysis of water, hydrogen obtained from the hydride, or hydrogen obtained from the metal-hydrogen solution. In another embodiment, the hydrogen molecules in the energy-emitting material 56 are dissociated into hydrogen atoms by the hydrogen molecule dissociation catalyst of the mixture 54. [ The dissociation catalyst is capable of absorbing hydrogen, deuterium, tritium atoms and / or molecules, and is capable of absorbing, for example, elements, compounds, refractory metals such as noble metals such as palladium and platinum, molybdenum and tungsten, Transition metals such as titanium, internal transition metals such as niobium and zirconium, and other materials mentioned in Mills prior art. Preferably, the dissociating agent has a surface area as high as a noble metal such as Pt, Pd, Ru, Ir, Re or Rh or Al ₂ O ₃ , Ni on SiO ₂ , or a combination thereof.

In one embodiment, the catalyst is provided by ionization of the t electrons to a continuous energy level wherein the sum of the ionization energies of the t electrons from the atom or ion is approximately m · 27.2 eV (where t and m are each an integer) . The catalyst may also be provided by transferring t electrons between the participating ions. The transfer of t electrons from one ion to another provides the net enthalpy of the reaction so that the value obtained by subtracting the ionization energy of the t electron of the electrons that receive electrons from the t ionization energy of the electrons gives m 27.2 eV (Where t and m are integers, respectively). In another preferred embodiment, the catalyst comprises MH, such as NaH, with M atoms bonded to hydrogen, and m 27.2 eV is provided as the sum of the M-H bond energy and the ionization energy of t electrons.

In a preferred embodiment, the catalyst bed comprises a catalytic material 58 fed through a catalyst feed path 41, and generally provides a net enthalpy of about ± 1 eV. The catalysts can be prepared by reacting the atoms listed in the specification and described in Mills prior art (see, e.g., Table 4 of PCT / US90 / 01998 and 25-46, pages 80-108 of PCT / US94 / 02219) Ions, molecules, and hydrino. In an embodiment, the catalyst of AlH, BiH, ClH, CoH, GeH, InH, NaH, RuH, SbH, SeH, SiH, SnH, C _2, N _2, O _2, CO _2, NO ₂ and NO ₃ M and Pb are selected from the group consisting of Li, Be, K, Ca, Ti, V, Cr, Mn, Fe, Co, Ni, Cu, Zn, As, Se, Kr, Rb, Sr, Nb, Mo, Pd, Sn, Ce, Pr, Sm, Gd, Dy, Pb, Pt, Kr, 2K +, He +, Na +, Rb +, Sr +, Fe 3+, Mo 2+, Mo 4+, In 3+, He +, Atoms and ions of Ar.sup. ⁺ , Xe.sup. ⁺ , Ar.sup.2 ⁺ and H.sup. ⁺ , And at least one species selected from the group of Ne.sup. ⁺ And H.sup. ⁺ .

Hydrogen catalytic reactor and electric power system

In one embodiment of the power system, heat is removed by a heat exchanger having a heat exchange medium. The heat exchanger may be a water wall, and the medium may be water. Heat can be transferred directly for space and heating processes. Alternatively, the heat exchange medium such as water undergoes a phase change such as steam conversion. Such a conversion may occur in the steam generator. Steam can be used to generate electricity in heat engines such as steam turbines and generators.

 One embodiment of a hydrogen catalytic energy and low energy hydrogen species production reactor 5 for recycling or regenerating fuel according to the present invention is shown in Figure 2A, which includes a solid fuel mixture 11, a hydrogen source 12, a steam pipe, A boiler containing a steam generator 13, a power converter such as a turbine, a water condenser 16, a water-replenishing source 17, a solid fuel recycler 18 and a hydrogen-dihydrogen gas separator 19 10). In step 1, the solid fuel comprising the catalyst and the hydrogen source is reacted to form the hydrino and low energy hydrogen product. In step 2, the spent fuel is reprocessed and re-supplied to the boiler 10 to maintain thermal power generation. The heat generated in the boiler 10 forms steam in the pipe and steam generator 13 and is transferred to the turbine 14, which in turn generates electricity by operating the generator. In step 3, water is condensed by the water cooler 16. The water loss is made by the water source 17 to complete the cycle and maintain the heat-electric force conversion. In step 4, a low-energy hydrogen product such as a hydrino hydride compound and a dihydrin gas may be removed and the unreacted hydrogen may be returned to the fuel recycler 18 or the hydrogen source 12 and added back to the spent fuel Thereby replenishing the recycled fuel. The gaseous product and the unreacted hydrogen can be separated by the hydrogen-dihydrochloride gas separator 19. Any product hydrinos hydride compounds can be separated and removed using a solid-fuel recycler 18. The process may be performed either inside the boiler where the solid fuel returns or outside the boiler. Thus, the system may further comprise at least one gas and mass transfer device for moving the reactants and products to achieve the spent fuel removal, regeneration, and re-feeding. Hydrogen for replenishing the hydrogen used in the hydrino formation is added from the source 12 during fuel regeneration, which may include reused spent hydrogen. The recycled fuel maintains thermal power production and allows the power generation unit to produce electricity.

In a preferred embodiment, the reaction mixture is capable of producing a reactant of an atomic or molecular catalyst and a hydrogen atom that further reacts to form a hydrino, and the product species formed by the formation of the catalyst and atomic hydrogen, ≪ / RTI > In one embodiment, the reactor includes a moving bed reactor, which may further include a fluidization reactor section in which the reactants are continuously supplied and by-products are removed and regenerated and returned to the reactor. In one embodiment, a low-energy hydrogen product, such as a hydrino hydride compound or dihydrino molecule, is recovered as the reactant is regenerated. Furthermore, hydrino hydride ions can be converted to dihydrino molecules during the formation of other compounds or during regeneration of the reactants.

The power system may further comprise catalytic condenser means for maintaining the catalyst vapor pressure by means of a temperature regulating means for regulating the surface temperature to a temperature lower than the reaction cell. The surface temperature is maintained at the desired value to provide the desired catalyst vapor pressure. In one embodiment, the catalytic condenser means is an in-cell tube grid. In one embodiment of the heat exchanger, the flow rate of the heat exchange medium can be regulated at a rate that maintains the condenser at a lower preferred temperature than the main heat exchanger. In one embodiment, the working medium is water and the flow rate is higher in the cooler than the water wall, so that the condenser is at a lower and preferred temperature. Each stream of the working medium can be recombined to be transferred for space and thermal processing or conversion to steam.

This energy invention is further described in the Mills prior art incorporated by reference in the specification. The cell of the present invention includes those previously described and further includes the catalysts, reaction mixtures, methods, and systems disclosed herein. The present invention provides an electrolytic cell energy reactor, a plasma electrolysis reactor, a gas discharge energy reactor, a barrier electrode reactor, an RF plasma reactor, a pressurized gas energy reactor, a gas discharge energy reactor, a microwave cell energy reactor, and a glow discharge cell and microwave and / Combinations of RF plasma reactors include: a hydrogen source; One of the solid, molten, liquid and gaseous sources of the catalyst; Wherein the reaction to form the low energy hydrogen occurs by contacting the hydrogen with the catalyst or by the reaction of the MH catalyst. For power conversion, each cell type may be replaced by thermal energy or plasma as described in the Mills prior art, as well as transformers known to those skilled in the art such as thermal engines, steam or gas turbine systems, stairing engines or thermal ion or thermal power converters, And may be connected to any transducer that converts it to an electric force.

The additional plasma transducer may be a magnetic mirror magnetic fluid power converter, a plasmadynamic power converter, a gyrotron, a photon bunching microwave power converter, a charge drift power, And a photoelectric transducer.

In one embodiment, the cell includes a cylinder of at least one internal combustion engine as shown in the Mills prior art.

Hydrogen gas cells and solid fuel reactors

According to one embodiment of the present invention, the hydrinos and reactors for generating power can take the form of hydrogen gas cells. The gas cell hydrogen reactor of the present invention is shown in FIG. 3A. The hydrino reactant is provided by catalysis with the catalyst. The catalysis can take place in the gas phase or in solid or liquid state.

 The reactor of Figure 3A includes a reaction vessel 207 having a chamber 200 that may contain vacuum or atmospheric pressure. The hydrogen source 201 connected to the chamber 200 transfers hydrogen to the chamber through the hydrogen supply path 242. The regulator 222 is positioned to regulate the pressure and flow of hydrogen entering the vessel through the hydrogen feed path 242. The pressure sensor 223 monitors the pressure in the container. Vacuum pump 256 is used to remove air from the chamber through vacuum tube 257.

In one embodiment, the catalysis occurs on a gas phase. The catalyst is gasified by maintaining the cell temperature at a high temperature and alternately determines the air pressure of the catalyst. The atomic and / or molecular hydrogen reactant may also be maintained at the desired pressure, which may range anywhere within the field. In one embodiment, the pressure is in a range of less than air pressure, preferably from about 10 mTorr to about 100 mTorr. In yet another embodiment, the pressure is determined by maintaining a mixture of a corresponding hydride, such as a metal hydride, and a catalyst source, such as a metal source, in a cell maintained at the desired operating temperature.

A catalyst source 250 for generating hydrino atoms may be placed in the catalyst reservoir 295 and a gaseous catalyst may be formed by heating. The reaction vessel 207 has a catalyst supply path 241 for passage of the gaseous catalyst from the catalyst reservoir 295 to the reaction chamber 200. Alternatively, the catalyst may be placed in an open chemical-resistant container such as a boat inside the container.

The hydrogen source may be hydrogen gas and molecular hydrogen. Hydrogen can be dissociated into hydrogen atoms by a molecular hydrogen dissociation catalyst. The dissociation catalyst or dissociation agent includes, for example, Raney nickel (R-Ni), a valuable metal or a noble metal, a valuable metal on the support or a noble metal. The oil or noble metal may be Pt, Pd, Ru, Ir, and Rh, and the support may be at least one of Ti, Nb, Al ₂ O ₃ , SiO _2, and combinations thereof. Additional dissociation agents include, but are not limited to, hydrogen spillover catalysts, nickel fiber mats, Pd sheets, Ti sponges, Ti or Ni sponges, or electroplated Pt or Pd, TiH, Pt black, and Pd black, molybdenum, and tungsten Transition metals such as refractory metals, nickel and titanium, and Pt or Pd on carbon which may include other such materials mentioned in previous Mills prior art documents. In a preferred embodiment, the hydrogen dissociates on Pt or Pd. The Pt or Pd may be coated on a support material such as titanium or Al ₂ O ₃ . In another embodiment, the dissociation agent is a refractory metal such as tungsten or molybdenum, and the dissociation material is elevated by temperature regulation means 230, which can take the form of a heating coil, as shown in the cross- Lt; / RTI > The heating coil is powered by a power supply 225. Preferably, the dissociation material is maintained at the operating temperature of the cell. The dissociation agent can be further activated at a temperature above the cell temperature to more effectively dissociate, and the rising temperature can prevent the catalyst from condensing on the dissociation agent. The hydrocracker may also be provided by a hot filament, such as 280, powered by a feeder 285.

In one embodiment, hydrogen dissociation occurs and the dissociated hydrogen atom contacts the gaseous catalyst to produce the hydrino atom. The catalyst vapor pressure is maintained at the desired pressure by regulating the temperature of the catalyst reservoir 295 to the catalyst reservoir heater 298 powered from the power supply 272. When the catalyst is contained in a boat inside the reactor, the catalyst vapor pressure is adjusted to the desired value by adjusting the temperature of the catalyst boat by regulating the power source of the boat. The cell temperature can be regulated at a desired operating temperature by the heating coil 230 powered by the power supply 225. The cell (also referred to as a permeable cell) may further include an internal reaction chamber 200 and an external hydrogen reservoir 290 to allow hydrogen to be supplied to the cell by hydrogen diffusion through a wall 291 separating the two chars have. The temperature of the wall can be adjusted with a heater to adjust the diffusion rate. The diffusion rate can be further controlled by adjusting the hydrogen pressure in the hydrogen reservoir.

To keep the catalyst pressure at a desired level, a cell with permeation, such as a hydrogen source, can be sealed. Alternatively, the cell may further include a high temperature valve at each injection or discharge, such that the valve in contact with the reactant gas mixture is maintained at the desired temperature. The cell may further include a getter or trap 225 that selectively collects hydrogen compounds with increased low energy hydrogen species and / or binding energies, and may include a selective valve (s) to release dihydrogen gas product (206). ≪ / RTI >

The catalyst may comprise at least one or more of the group of lithium atoms, potassium atoms or cesium atoms, NaH molecules and hydrino atoms, wherein the catalytic action involves a disproportion reaction. The lithium catalyst becomes a gas by maintaining the cell temperature in the range of 500-1000 ° C. Preferably the cell is maintained in the range of 500-750 < 0 > C. The cell pressure may be maintained at less than atmospheric pressure, preferably in the range of about 10 mTorr to about 100 Torr. Most preferably, at least one of the catalyst and hydrogen pressure is selected from the group consisting of lithium and lithium hydride, potassium and potassium hydrides, sodium and sodium hydrides, and mixtures of catalyst metals and corresponding hydrides, such as cesium and cesium hydrides, Lt; RTI ID = 0.0 > operating temperature. ≪ / RTI > The gas phase catalyst may comprise a lithium atom from a metal or lithium metal source. Preferably, the lithium catalyst is maintained at a pressure determined by a mixture of a lithium metal and a lithium hydride in an operating temperature range of 500-1000 DEG C, most preferably a cell having an operating temperature range of 500-750 DEG C . In another embodiment, K, Cs, and Na replace Li, wherein the catalyst is a K atom, a Cs atom, and a NaH molecule.

One embodiment of a gas cell reactor comprising a catalyst reservoir or boat, a gaseous Na, NaH catalyst, or a gaseous catalyst such as Li, K, and Cs vapor, and is maintained in a super-heated condition. In one embodiment, the superheated steam reduces the condensation of the catalyst on the dissociation agent of at least one of the hydrogen dissociation agent or the metal and metal hydride molecules disclosed in infra. In an embodiment comprising Li as a catalyst from a reservoir or a boat, the reservoir or boat is maintained at a temperature at which Li evaporates. H ₂ is maintained at a pressure lower than the pressure at which LiH forms a steep molar fraction at the reservoir temperature. The pressure and temperature achieving this condition can be determined from a data line such as Mueller as shown in Figure 6.1 [40] of H ₂ pressure versus LiH mole fraction at a given isotherm. In one embodiment, the cell reaction chamber containing the dissociation agent is operated at a high temperature such that Li does not condense on the walls or dissociation agent. H ₂ can flow from the reservoir to the cell to increase the rate of catalyst delivery. The flow out of the cell after flowing from the catalyst reservoir to the cell is a means of removing the hydrino product and preventing the hydrinos from inhibiting the reaction. In another embodiment, K, Cs, and Na replace Li, where the catalyst is a K atom, a Cs atom, and a NaH molecule.

Hydrogen is supplied to the reaction from a hydrogen source. Preferably, hydrogen is supplied by the permeable membrane from the hydrogen reservoir. The pressure of the hydrogen reservoir may be in the range of 10 Torr to 10,000 Torr, preferably 100 Torr to 1000 Torr, and most preferably at about atmospheric pressure. The cell may be operated at a temperature of about 100 ° C to 3000 ° C, preferably about 100 ° C to 1500 ° C, and most preferably about 500 ° C to 800 ° C.

The hydrogen source may be from decomposition of the added hydride. The cell design that supplies H ₂ by the permeable membrane is comprised of an internal metal hydride located in a sealed vessel where the H atoms permeate at high temperatures. The vessel may comprise Pd, Ni, Ti or Nb. In one embodiment, the hydride is located in a sealed tube, such as an Nb tube containing hydride, and is sealed at both ends with a sealing device such as Swagelock. In the sealed case, the hydride may be an alkaline or alkaline earth hydride. Alternatively, as with the inner-hydride-reagent case, the hydrides can include saline hydride, titanium hydride, vanadium, niobium and tantalum hydride, zirconium and hafnium hydride, rare earth hydride, yttrium and scandium Hydrides, transition metal hydrides, intermetalic hydrides and at least one of the group of alloys suggested by WM Mueller et al. [40].

In one embodiment, based on the decomposition temperature of each hydride, the hydride and the operating temperature ± 200 ° C is at least one of the following list:

Rare earth hydrides having an operating temperature of 800 < 0 >C; A lanthanum hydride having an operating temperature of 700 캜; A gadolinium hydride having an operating temperature of 750 캜; A neodymium hydride having an operating temperature of 750 캜; Yttrium hydride having an operating temperature of 800 ° C; A scandium hydride having an operating temperature of 800 < 0 >C; A ytterbium hydride having an operating temperature of 850-900 캜; A titanium hydride having an operating temperature of about 450 < 0 >C; A cerium hydride having an operating temperature of about 950 캜; A praseodymium hydride having an operating temperature of about 700 캜; Zirconium-titanium (50% / 50%) hydride having an operating temperature of about 600 ° C; An alkali metal / alkali metal hydride mixture such as Rb / RbH or K / KH having an operating temperature of about 450 < 0 >C; And Ba / BaH alkaline earth metals, such as ₂ / alkaline earth hydride mixture having an operating temperature of about 900-1000 ℃.

The gaseous metal comprises a divalent covalent molecule. It is an object of the present invention to provide atomic catalysts such as Li as well as K and Cs. Thus, the reactor may further comprise at least one dissociating agent of metal molecules (" MM ") and metal hydride molecules (" MH "). Preferably, the catalyst source, the H ₂ source, and the dissociation agent of MM, MH and HH, where M is an atomic catalyst, are matched for operation at the desired cell conditions, for example, temperature and reactant concentration. In one embodiment, when a H ₂ hydride source is used, its decomposition temperature is within a range of temperatures that produce a vapor pressure of the desired catalyst. When the hydrogen source is permeated from the hydrogen reservoir to the reaction chamber, the preferred catalyst sources for continuous operation are Sr and Li, since their respective vapor pressures are within the desired range of 0.01 to 100 Torr at the temperature at which permeation takes place. In another embodiment of the transmissive cell, the cell is operated at a high temperature that allows permeation, then the cell temperature is lowered to a temperature that maintains the vapor pressure of the volatile catalyst at the desired pressure.

In one embodiment of the gas cell, the dissociation agent comprises means for producing a catalyst and H from a source. Surface catalysts such as Pt on Ti or Pd, alone or iridium or rhodium on a substrate such as Ti, also function as dissociating agents for the molecules in which the catalyst and atomic hydrogen are combined. Preferably, the dissociating agent has a high surface area such as Pt / Al ₂ O ₃ orPd / Al ₂ O ₃ .

The H ₂ source can also absorb H ₂ gas. In this case, the pressure is observed and adjusted. This is possible with catalysts and catalyst sources such as K or Cs metal and LiNH ₂ , respectively, because they volatilize at low temperatures, allowing the use of high temperature valves. LiNH ₂ also allows long-duration operation by lowering the required operating temperature of the Li cell and injecting it through the interior of the plasma and filament cell case where the filaments act as a hydrogen dissociating agent because of the low corrosion.

A further embodiment of a gaseous-cell hydrogen reactor with NaH as catalyst comprises a dissociation agent in the reactor cell and a filament with Na in the reservoir. H ₂ can flow into the main chamber through the reservoir. Power is regulated by adjusting the gas flow rate, H ₂ pressure and Na vapor pressure. The latter can be adjusted by adjusting the reservoir temperature. In yet another embodiment, the hydrino reaction is initiated by heating with an external heater, and the H atom is supplied by a dissociation agent.

The present invention also relates to other reactors for producing hydrogen compounds with increased binding energy of the present invention such as dihydrino molecules and hydrino hydride compounds. Additional products of catalysis are plasma, light and power. The reactor is hereinafter referred to as a " hydrogen reactor " or " hydrogen cell ". The hydrogen reactor comprises a cell for making hydrinos. The cell for making the hydrinos can take the form of, for example, a gas cell, a gas discharge cell, a plasma torch cell or a microwave power cell. These exemplary cells are disclosed in the Mills prior art document and are incorporated by reference. Each such cell comprises a hydrogen atom source; At least one of a solid, molten or gaseous catalyst for making hydrinos; And a vessel for reacting hydrogen and a catalyst for making the hydrinos. As used and discussed in this specification, the term "hydrogen" includes deuterium ( ² H) and tritium ( ³ H) as well as proteases ( ¹ H) .

Hydrogen gas discharge power and plasma cell and reactor

The hydrogen gas discharge power and plasma cell and reactor of the present invention are shown in FIG. 4A. The hydrogen gas discharge power and plasma cell and reactor of FIG. 4A include a gas discharge cell 307 including a glow discharge vacuum vessel 355 filled with a hydrogen gas having a chamber 300. The hydrogen supply source 322 supplies hydrogen to the chamber 300 through the regulating valve 325 by the hydrogen supply path 342. The catalyst is contained in the cell chamber 300. The voltage and current source 330 allows current to pass between the anode 305 and the cathode 320. The current may be reversible.

In one embodiment, the material of the anode 305 may be a catalyst source such as Fe, Dy, Be or Pd. In another embodiment of the hydrogen gas discharge power and plasma cell and reactor, the walls of the vessel 313 are conductive and serve as an anode to replace the electrode 305, and the cathode 320, like a stainless steel hollow cathode, May be open. The discharge can evaporate the catalyst source to the catalyst. The hydrogen molecule may dissociate by discharge to form hydrino and hydrogen atoms for generating energy. Additional dissociation can occur by in-chamber hydrogen dissociation.

Another embodiment of the hydrogen gas discharge power and plasma cell and reactor in which the catalyst takes place in the gas phase utilizes an adjustable gas catalyst. The gaseous hydrogen atoms to be converted to the hydrino are provided by the discharge of the hydrogen molecular gas. The gas discharge cell 307 has a catalyst supply path 341 for passing the gas catalyst 350 from the catalyst reservoir 395 to the reaction chamber 300. The catalyst reservoir 395 is heated by a catalyst reservoir heater 392 having a power supply 372 for supplying a gaseous catalyst to the reaction chamber 300. The catalyst vapor pressure is regulated by regulating the heater 392 by the power supply 372 to regulate the temperature of the catalyst reservoir 395. The reactor further comprises a selective venting valve (301). An open container that is chemically resistant, such as stainless steel, tungsten, or ceramic boat, and located within a gas discharge cell, may include a catalyst. The catalyst in the catalyst boat may be heated with a boat heater using an associated power supply to provide a gaseous catalyst to the reaction chamber. Alternatively, the glow gas discharge cell is operated at an elevated temperature such that the catalyst in the boat is sublimed, boiled, or evaporated to become a gaseous phase. To prevent the catalyst from condensing in the cell, the temperature is maintained above the temperature of the catalyst source, the catalyst reservoir 395, or the catalytic boat.

In a preferred embodiment, the catalysis takes place in the gas phase, lithium is the catalyst, and a lithium atom source such as lithium metal or a lithium compound such as LiNH ₂ is gasified by maintaining the cell temperature in the range of about 300-1000 ° C . More preferably the cell is maintained in the range of about 500-750 < 0 > C. The atomic and / or molecular hydrogen reactant is maintained at a pressure below atmospheric pressure, preferably in the range of about 10 mTorr to about 100 Torr. Most preferably, the pressure is determined by maintaining a mixture of a lithium metal and a lithium hydride in a cell maintained at a desired operating temperature. The operating temperature range is preferably in the range of 300-1000 ° C, and most preferably the pressure is achieved in a cell at an operating temperature of about 300-750 ° C. The cell can be regulated to a desired operating temperature by a heating coil, such as 380 of Figure 4A, powered by a power supply 385. [ The cell may further include an inner reaction chamber 300 and an outer hydrogen reservoir 390 so that hydrogen can be supplied to the cells by diffusing the hydrogen through the wall 313 separating the two chambers. The temperature of the wall can be controlled by a heater that adjusts the diffusion rate. The diffusion rate can be further controlled by adjusting the hydrogen pressure in the hydrogen reservoir.

One embodiment of the plasma cell of the present invention regenerates reactants such as Li and LiNH ₂ . In one embodiment, the reaction given by equations (32) and (37) takes place to produce the hydrino reactants, Li and H, with a significant excess of energy released due to hydrino production. The product is then hydrogenated by a hydrogen source. When LiH is formed, one reaction to produce a low-energy hydrogen-catalyzed reactant is shown in equation (66). This can be accomplished with a reactant located within the reaction zone within the plasma cell, such as in the anode region within the hydrogen plasma cell. The reaction is LiH + e- - may be 30, and ^{_{thereafter, Li 2 NH + H - -}} > Li and _{H -> Li + LiNH 2 (} 31) the reaction is somewhat up in the normal state Li + LiNH ₂ (steady-state) level. The pressure, electron density, and energy may be adjusted to achieve a maximum or desired reaction to produce the hydrinot reactant Li + LiNH ₂ .

In one embodiment, the mixture is stirred or mixed during the plasma reaction. In a further embodiment of the plasma regeneration system and method of the present invention, the cell comprises a heated, flat-bottomed stainless steel plasma chamber. LiH and Li ₂ NH include Li molten mixture. Since stainless steel is not magnetic, the stainless steel coated stirrer driven by a stirring motor installed in a flat-bottom plasma reactor can immediately stir the liquid mixture. The Li-metal mixture can act as an anode. Reduction of LiH to Li and the further reaction of H & lt ^; + > Li ₂ NH with Li and LiNH ₂ can be monitored by XRD and FTIR of the product. In another embodiment of _{Li, LiNH 2, Li 2 NH} , Li 3 N, LiNO 3, LiX, NH 4 X (Xisahalide), NH 3, and H system with a reaction mixture containing a species of a group of ₂ , At least one of the reactants is regenerated by addition of one or more reagents and by plasma regeneration. Plasma is NH ₃ and H ₂ . Or the like. Plasma can be held in place (in the reaction cell) or in an external cell that communicates with the reaction cell. In another embodiment, K, Cs, and Na replace Li, where the catalyst is a K atom, a Cs atom, and a NaH molecule.

To keep the catalyst pressure at a desired level, a cell having permeation, such as a hydrogen source, can be sealed. Alternatively, a high temperature valve is additionally included in each inlet or outlet so that the valve in contact with the reactant gas mixture is maintained at the desired temperature.

The plasma cell temperature can be adjusted independently and broadly by isolating the cell and supplying supplemental heater power to the heater 380. Thus, the catalyst vapor pressure can be adjusted independently of the plasma power.

The discharge voltage is in the range of about 100 to 10,000 volts. The current may be within any desired range at the desired bolt. Further, the plasma may be pulsed as disclosed in the Mills prior art, such as PCT / US04 / 10608 (entitled "Pulsed Plasma Power Cell and Novel Spectral Lines"), which is incorporated herein by reference.

Boron nitride may include a feed-through of the plasma cell because the material is stable to Li vapor. Crystalline or transparent alumina is another stable feed-through material of the present invention.

Solid fuel and hydrogen catalytic reactors

The gaseous metal comprises a divalent covalent molecule. It is an object of the present invention to provide K and Cs as well as atomic catalysts such as Li and molecular catalyst NaH. Thus, in one embodiment of the solid-fuel, the reactant comprises a source of a complex that reversibly forms and decomposes or reacts with the alloy, complex or metal catalyst M to provide a gaseous catalyst such as Li. In yet another embodiment, at least one of the catalyst source and the hydrogen atom source further comprises at least one reactant to form at least one of a catalyst and an atomic hydrogen. In one embodiment, the source comprises at least one of an amide such as LiNH ₂ , an imide such as Li ₂ NH, a nitride such as Li ₃ N, and a catalytic metal with NH ₃ . These and other embodiments are given in infra. Where further K, Cs, and Na can replace Li, and the catalyst is a K atom, a Cs atom, and a NaH molecule.

The present invention relates to an energy reactor comprising an energy reactor comprising a reaction vessel constructed and arranged to contain a pressure lower than, equal to or higher than atmospheric pressure, a hydrogen atom source for chemically producing a hydrogen atom in communication with the vessel, A catalyst source comprising at least one of an atom, a cesium atom, a potassium atom and a NaH molecule, and may further comprise a getter, such as a source of an ionic compound for binding or reacting with a low energy hydride. Catalysts and Reactants The source of hydrogen atoms can include solid fuels that are continuously or batch regenerated inside or outside the cell where the H catalysis and the physical process or chemical reaction to form hydrinos Catalyst and H from the source. Thus, embodiments of the hydrino reactants of the present invention include a solid fuel, and preferred embodiments include a solid fuel that can be regenerated. Solid fuels may be used in a variety of applications, including space and process heating, electricity generation, power generation, propellant, and other applications that are well known to those skilled in the art.

The gas cell or plasma cell of the present invention as shown in Figures 3A and 4A includes means for forming a catalyst and H from a source. In a solid-fuel embodiment, the cell further comprises a reactant to provide a catalyst and H when initiating a chemical or physical process. The process is initiated by means such as heating or plasma reaction. Preferably, the need for external power to maintain hydrinogenation is low or very low compared to the large power of the H catalytic reaction that produces hydrinos. Reactants can be regenerated with net emission energy for reaction and regeneration.

In another embodiment, the reactor shown in Figure 3A comprises a solid fuel reactor, wherein the reaction mixture comprises a catalyst source and a hydrogen source. The reaction mixture can be regenerated by feeding the flow of reactant and removing the product from the corresponding product mixture. In one embodiment, the reaction vessel 207 has a chamber 200 that can contain a vacuum or atmospheric pressure equal to or greater than atmospheric pressure. At least one reagent source, such as a gaseous reagent 221, is in communication with the chamber and delivers the reagent to the chamber through at least one reagent supply path 242. The controller 222 is arranged to regulate the pressure of the reagent and the flow of the reagent through the reagent supply path 242 to the vessel. A vacuum pump 256 is used to evacuate the chamber through the vacuum line 257. Alternatively, line 257 represents at least one outlet, such as a product path line that removes material from the reactor. The reactor further comprises a source of heat, such as a heater 230 for raising the reactants to a desired temperature to initiate solid fuel chemistry and hydrino formation catalysis. In one embodiment, the temperature is in the range of about 50 to 1000 占 폚, preferably about 100 to 600 占 폚, and for reactants comprising at least the Li / N-Alloy system, the desired temperature is 100 to 500 占 폚 Range.

The cell may further comprise a hydrogen gas source and a dissociation agent to form hydrogen atoms of the hydrogen gas. The vessel may further comprise a hydrogen source (221) in communication with a vessel for producing at least one of an atomic catalyst source such as a lithium atom and a hydrogen atom source. The hydrogen source may be hydrogen gas. H ₂ gas may be supplied by hydrogen line 242 from hydrogen reservoir 290 or by permeation. In an exemplary regeneration reaction, the source of lithium atoms and atomic hydrogen may be regenerated by hydrogenation according to equation (66-71). The first step of the alternative regeneration reaction can be given in equation (69).

In one embodiment, the cell size and material are such that high operating temperatures are recorded. The cell may be suitably fabricated to fit the power outlet to achieve the desired operating temperature. High temperature materials for cell fabrication are high temperature stainless steel such as niobium and Hastalloy. The H ₂ source may be an internal metal hydride that does not react with LiNH ₂ but releases only H at very high temperatures. In addition, the number of the hydride can be separated from the reagent, such as Li and LiNH ₂ When the reaction LiNH _2, by placing in a cell in an open or a closed container. The cell design that supplies H ₂ by permeation includes an inner metal hydride disposed in a sealed vessel where hydrogen atoms permeate at high temperatures.

The reactor may further comprise means for separating the components of the product mixture, such as a sieve that mechanically separates by a difference in physical properties, such as size. The reactor may further comprise means for separating one or more components based on a phase change or reaction difference. In one embodiment, the phase change comprises melting using a heater, wherein the liquid is separated from the solid by means known in the art, such as gravity filtration, filtration through a pressurized gas, and centrifugation. The reaction may involve decomposition, such as decomposition of the hydride, which may be carried out by dissolving the corresponding metal respectively, separating them, or mechanically separating the hydrides. The latter can be achieved by sieving. In one embodiment, the phase change or reaction may produce the desired reactants or intermediates. In an embodiment, regeneration, including any desired separation step, may occur within or outside the reactor.

Chemical reactor

The chemical reactor of the present invention further comprises a source of inorganic compounds such as MX, where M is an alkali metal and X is a halide. In addition to the hydrides, inorganic compounds include alkali earth salts such as alkali or hydroxides, oxides, carbonates, sulphates, phosphates, borates and silicates (other suitable inorganic compounds are described in DR Lide, CRC Handbook for example, in Chemistry and Physics, 86th Edition, CRC Press, Taylor & Francis, Boca Raton, (2005-6), pp.4-45 to 4-97. Inorganic compounds can additionally act as getters to produce power or to inhibit other products by preventing product accumulation and the adverse reaction thereto. Preferred Li chemical- include Li, LiNH _2, LiBr or LiI and R-Ni in the type of power selneun hydrogen cell operating at about 760 Torr H ₂ and about 700 + ℃. Preferred NaH chemical- and Na, NaX in the hydrogen cell operating at power selneun about 760 Torr H ₂ and about + 700 ℃ of type (X is a halogen the cargo, being preferably Br or I) and include the R-Ni. The cell may further include at least one of the cells. Preferred chemical K-type and power selneun including K, KI, and Ni screen or R-Ni in the hydrogen dissociation the cell operating at about 760 Torr H ₂ and about 700 + ℃. In one embodiment, the H ₂ pressure range is from about 1 Torr to 10 ⁵ Torr. Preferably, the hydrogen is maintained in the range of about 760-1000 Torr. LiHX, such as LiHBr and LiHI, is generally synthesized in the temperature range of about 450-550 DEG C, but can be operated at a lower temperature (~ 350 DEG C) with existing LiH. NaHBr and NaHI are generally synthesized in the temperature range of about 450-550 < 0 > C. KHX, such as KHI, is synthesized in the temperature range of about 450-550 ° C. In the NaHX and KHX reactor embodiments, NaH and K are supplied from a source such as a catalyst reservoir wherein the cell temperature is maintained at a higher level than the catalyst reservoir. Preferably, the cell is maintained at a temperature in the range of about 300-500 < 0 > C, and the reservoir is maintained in a temperature range of about 50 to 200 < 0 > C or less.

Another embodiment of a hydrogen reactor having NaH as the catalyst is a plasma torch for the generation of hydrogen compounds with increased binding energy such as power and NaHX where H is hydrogen with increased binding energy and X is a halide. . At least one of NaF, NaCl, NaBr, NaI may be sprayed in a plasma gas such as rare gas (noble gas) / hydrogen mixture such as H ₂ or He / H ₂ or Ar / H _2.

General Solid Fuel Chemistry

The reaction mixture of the present invention comprises a catalyst or a catalyst source and a hydrogen atom or an atomic hydrogen (H) source, wherein at least one of the catalyst and the hydrogen atom is reacted by a chemical reaction between one or more reaction mixture species or two or more reaction mixture species . Preferably, the reaction is reversible. Preferably, the released energy is greater than the enthalpy of the formation reaction of the catalyst and the reactant hydrogen, and preferably when the reactant of the reaction mixture is regenerated and recycled, preferably the product H of the product H given by equation (1) Formation energy releases net energy over the course of the reaction and regeneration. The species may be one or more of an element, an alloy or a compound such as a molecule or an organic compound, each of which may be one or more of the reactants or products in the reactor. In one embodiment, the species may form an alloy or compound such as a molecule or an organic compound with at least one of hydrogen and a catalyst. The at least one reaction mixture species forms one or more reaction product species such that the release energy of H or free catalyst is relatively lower than in the absence of formation of the reaction product species. In embodiments where the reactant provides a catalyst and atomic hydrogen to form a state having an energy level given by equation (1), the reactant includes at least one of solid, liquid (including molten) and gaseous reactants . The reaction to form the catalyst and the atomic hydrogen to form a state having the energy level given by equation (1) occurs in at least one of the solid, liquid (including molten state) and gas phase. The exemplary solid-fuel reactions presented herein are not meant to be strictly limiting, as other reactions, including additional reagents, are also within the scope of the present invention.

In one embodiment, the reaction product species is at least one of the catalyst and hydrogen or a source thereof. In one embodiment, the reaction mixture species is a catalytic hydride and the reaction product species is a catalytic alloy or compound having a relatively low hydrogen content. The energy that releases H from the hydride of the catalyst may be lowered by the formation of an alloy or a second compound with one or more other species such as an element or a first compound. In one embodiment, the catalyst is one of Li, K, Cs and NaH molecules, and the hydride is one of LiH, KH, CsH and NaH and the at least one other element is selected from the group consisting of M (catalyst) Si, C, N, Sn, Te, P, S, Ni, Ta, Pt and Pd. Wherein the first and second compounds are selected from the group consisting of H ₂ , H ₂ O, NH ₃ , NH ₄ X where X is a counterion such as halide and the other anions are described in DR Lide, CRC Handbook of Chemistry and Physics, 86th Edition, CRC Press , Taylor & Francis, Boca Raton, (2005-6), are given in pp.4-45 to 4-97], and incorporated by reference _{herein), MX, MNO 3, MAlH} 4, M 3 AlH 6, MBH ₄ , M ₃ N, M ₂ NH and MNH ₂ , where M is an alkali metal which may be a catalyst. In another embodiment, the hydride comprising at least one element other than the catalytic element releases H by reversible decomposition.

One or more reaction mixture species may form one or more reaction product species such that the free catalyst release energy is relatively lower than in the absence of formation of reaction product species. The reactive species such as alloys or compounds can release the free catalyst by reversible reaction or decomposition. In addition, the free catalyst can be formed by reversible reaction of the catalyst source with one or more other species such as elements or first compounds to form species such as alloys or second compounds. The element or alloy may include at least one of M (catalytic atom), H, Al, B, Si, C, N, Sn, Te, P, S, Ni, Ta, Pt and Pd. The first and second compounds may be one of the group of H ₂ , NH ₃ and NH ₄ X, wherein M is an alkali metal which may be a catalyst. The catalyst may be one of Li, K and Cs atoms, and NaH molecules. The catalyst source may be MM, such as LiLi, KK, CsCs, and NaNa. The H source may be MH, such as LiH, KH, CsH or NaH.

The Li catalyst can be allayed or reacted to form compounds with one or more other elements or compounds to lower the energy barrier to Li release from LiH, or LiH and LiLi molecules. In addition, the alloy or compound may release H or Li by decomposition or reaction with additional reactive species. The alloy or compound may be one or more of the group of LiAlH ₄ , Li ₃ AlH ₆ , LiBH ₄ , Li ₃ N, Li ₂ NH, LiNH ₂ , LiX and LiNO ₃ . The alloy or compound may be at least one of Li / Ni, Li / Ta, Li / Pd, Li / Te, Li / C, Li / Si and Li / Sn, The Li and H can be released optimally according to the change of the equivalence ratio between hydrogen and hydrogen, which then reacts during the catalytic reaction to form hydrogen in a relatively low energy state. In another embodiment, K, Cs, and Na replace Li, wherein the catalyst is a K atom, a Cs atom, and a NaH molecule.

In one embodiment, the alloy or compound has the formula M _x E _y , where M is a catalyst such as Li, K or Cs or Na, E is another element, x and y represent equivalence ratios. M and E _y can be any desired molar ratio. In one embodiment, x ranges from 1 to 50, y ranges from 1 to 50, preferably x ranges from 1 to 10, and y ranges from 1 to 10.

In another embodiment, the alloy or compound has the formula M _x E _y E _z , where M is a catalyst such as Li, K or Cs or Na, E _y is the first other element, E _z is the second And x, y and z represent equivalence ratios. M, E _y and E _z can be any desired molar ratios. In one embodiment, x ranges from 1 to 50, y ranges from 1 to 50, z ranges from 1 to 50, preferably x ranges from 1 to 10, y ranges from 1 to 10, z is 1 to 10. In a preferred embodiment, E _y and E _z are selected from the group of H, N, C, Si and Sn. The alloy or compound may be selected from the group consisting of Li _x C _y Siz, Li _x Sn _y Si _z , Li _x N _y Si _z , Li _x Sn _y C _z , Li _x N _y Sn _z , Li _x C _y N _z , Li _x C _y H _z , Li _x Sn _y H _z , Li _x N _y H _z, and Li _x Si _y H _z . In another embodiment, K, Cs, and Na replace Li, wherein the catalyst is a K atom, a Cs atom, and a NaH molecule.

In another embodiment, the alloy or the compound has the formula M _x E _w E _y E _z, where M is a catalyst for example, Li, K or Cs, or or Na and, E _w is the first other elements, E _y is E _z is the third different element, and x, w, y and z represent the equivalence ratio. M, E _y , E _y and E _z may be any desired molar ratios. In one embodiment, x ranges from 1 to 50, w ranges from 1 to 50, y ranges from 1 to 50, z ranges from 1 to 50, preferably x ranges from 1 to 10, and w is 1 to 10, y ranges from 1 to 10, and z ranges from 1 to 10. In a preferred embodiment, E _w , E _y and E _z are selected from the group of H, N, C, Si and Sn. The alloy or compound may be selected from the group consisting of Li _x H _w C _y Si _z , Li _x H _w Sn _y Si _z , Li _x H _w N _y Si _z , Li _x H _w Sn _y C _z , Li _x H _w N _y Sn _z , Li _x H _w C _y N _z . In another embodiment, K, Cs, and Na replace Li, wherein the catalyst is a K atom, a Cs atom, and a NaH molecule. Species such as M _x E _w E _y E _z are not meant to be limiting and other species, including additional elements, are also within the scope of the present invention.

In one embodiment, the reaction contains a hydrogen atom source and a Li catalyst source. The reaction is hydrogen dissociation claim, H _2, a source of hydrogen _{atom, Li, LiH, LiNO 3,} LiNH 2, Li 2 NH, Li 3 N, LiX, NH 3, LiBH 4, LiAlH 4, Li 3 AlH 6, NH 3 And NH ₄ X, wherein X is a counterion such as halide and CRC [41]. The wt% of the reactants may be in any desired molar range. The reactants can be mixed well using a ball mill.

In one embodiment, the reaction mixture comprises a catalyst source and a H source. In one embodiment, the reaction mixture further comprises a Li catalyst and a reactant that performs the reaction to form atomic hydrogen. The reactants include H ₂ , a hydrinocatalyst, MNH ₂ , M ₂ NH, M ₃ N, NH ₃ , LiX, NH ₄ X (where X is a counterion such as a halide), MNO ₃ , MAlH ₄ , M ₃ AlH ₆ And MBH ₄ , wherein M is an alkali metal, which may be a catalyst. The reaction mixture is _{Li, LiH, LiNO 3, LiNO} , LiNO 2, Li 3 N, Li 2 NH, LiNH 2, LiX, NH 3, LiBH 4, LiAlH 4, Li 3 AlH 6, LiOH, Li 2 S, LiHS , Li ₂ CO ₃ , LiHCO ₃ , Li ₂ SO ₄ , LiHSO ₄ , Li ₃ PO ₄ , Li ₂ HPO ₄ , LiH ₂ PO ₄ , Li ₂ MoO ₄ , LiNbO ₃ , Li ₂ B ₄ O _{7 tetraborate), LiBO 2, Li 2 WO} 4, LiAlCl 4, LiGaCl 4, Li 2 CrO 4, Li 2 Cr 2 O 7, Li 2 TiO 3, LiZrO 3, LiAlO 2, LiCoO 2, LiGaO 2, Li 2 GeO ₃ , LiMn ₂ O ₄ , Li ₄ SiO ₄ , Li ₂ SiO ₃ , LiTaO ₃ , LiCuCl ₄ , LiPdCl ₄ , LiVO ₃ , LiIO ₃ , LiFeO ₂ , LiIO ₄ , LiClO ₄ , LiScO _n , LiTiO _n , LiVO _n , LiCrO _n, LiCr ₂ O _n, LiMn ₂ O _n, LiFeO _n, LiCoO _n, LiNiO _n, LiNi ₂ O _n, LiCuO _n and LiZnO _n (here, n is 1, 2, 3 or 4) oxide anion (oxyanion , Oxidizing anions of strong acids, oxidizing agents, molecular oxidants such as V ₂ O ₃ , I ₂ O ₅ , MnO ₂ , Re ₂ O ₇ , CrO ₃ , RuO ₂ , AgO, PdO, PdO ₂ , PtO, PtO ₂ and NH ₄ X where X is nitrate or other suitable anion given in CRC [41] And reagents selected from the group of reducing agents. In each case, the mixture further comprises a hydrogen or hydrogen source. In another embodiment, other dissociation agents may be used or not, wherein the hydrogen atoms and optionally the catalyst atoms are chemically produced by the reaction of the mixture species. In a further embodiment, the reactant catalyst may be added to the reaction mixture.

The reaction mixture may further comprise an acid such as H ₂ SO ₃ , H ₂ SO ₄ , H ₂ CO ₃ , HNO ₂ , HNO ₃ , HClO ₄ , H ₃ PO ₃ and H ₃ PO ₄ or an acid source, . The latter includes at least one of the group of SO ₂ , SO ₃ , CO ₂ , NO ₂ , N ₂ O ₃ , N ₂ O ₅ , Cl ₂ O ₇ , PO ₂ , P ₂ O ₃ and P ₂ O ₅ .

In one embodiment, the reaction mixture further comprises a reactant catalyst to produce a reactant that acts as a low-energy-hydrogen catalyst or a low-energy-hydrogen catalyst source and a hydrogen or hydrogen atom source. Suitable reactant catalysts include one or more of the acid, base, halide, metal, and free radical sources. The reactant catalyst may be a weak-base catalyst such as Li ₂ SO ₄ , a weak acid catalyst such as a solid acid such as LiHSO ₄ , a metal ion source such as TiCl ₃ or AlCl ₃ providing Ti ³⁺ and Al ³⁺ ions respectively, source, for example CoX ₂ (wherein, X is a halide such as Cl, this time is Co ²⁺ can form a radical O _2- reacts with O _2), the metal for example and preferably of from about 1 mol% concentration of Ni, Fe And a source of Co, X ^- ions (where X is a halide) such as Cl ^- or F ^- from LiX ^- , a free radical initiator / carrier source such as peroxide, an azo group compound and UV light.

In one embodiment, the reaction mixture for low-energy hydrogen is prepared by ionizing a hydrogen source, a catalyst source, and a catalyst to resonate energy from the hydrogen atom to form a hydrinos having the energy given by equation (1) And one or more hydrinogetters from the catalyst and an electronic getter. Hydrinogetor can combine with low-energy hydrogen to prevent reverse reactions to normal hydrogen. In one embodiment, the reaction mixture comprises a hydrinogen, such as LiX or Li ₂ X, where X is an anion from a halide or other anion such as CRC [41]. The electronic getter can perform one or more functions to receive electrons from the catalyst and stabilize the catalyst-ion intermediate such as Li ^{2 +} intermediate to cause the catalytic reaction to occur at a high rate. The getter may be an inorganic compound comprising at least one cation and at least one anion. The cation may be Li < ⁺ >. The anion may be a halide or other anion given in CRC [41] such as F ^- , Cl ^- , Br ^- , I ^- , NO ₃ ^- , NO ₂ ^- , SO ₄ ^2- , HSO ₄ ^- , CoO ₂ ^- , IO ₃ ^- , IO ₄ ^- , TiO ₃ ^- , CrO ₄ ^- , FeO ₂ ^- , PO ₄ ^3- , HPO ₄ ^2- , H ₂ PO ₄ ^- , VO ₃ ^- , ClO ₄ ^- and Cr ₂ O ₇ ^2- One of the groups, and other anions in the reactants. The hydride binder and / or stabilizer may be one or more of the group LiX (X is a halide), and other compounds comprising the reactants.

In embodiments of the reaction mixture, such as Li, LiNH _2, and X where X is a hydride-binding compound, X is at least one of LiHBr, LiHI, a hydrino hydride compound and a low-energy hydrogen compound. In one embodiment, the catalytic reaction mixture is regenerated by hydrogenation from a hydrogen source.

In one embodiment, the hydrino product may be combined to form a stable hydrino hydride compound. The hydride binder may be LiX, where X is a halide or other anion. The hydride binder may react with a hydride having a higher NMR top field transition than an upfield shift of TMS. The binder may be an alkali halide and the hydride bonded product may be an alkali hydride with a higher NMR top field transition than the upper field transition of TMS. The hydride may have a binding energy determined by XPS of 11 to 12 eV. In one embodiment, the product of the catalytic reaction is a hydrogen molecule H ₂ (1/4) having a solid NMR peak at about 1 ppm for TMS and a binding energy of about 250 eV captured in the crystalline ion lattice. In one embodiment, the product H ₂ (1/4) is captured in the crystalline lattice of the ionic compound of the reactor such that the infrared absorption selectivity is such that the molecule is IR active and the FTIR peak is observed at about 1990 cm -1.

Additional Li atom sources of the present invention include additional Li alloys such as Li and one or more alkali metals, alkaline earth metals, transition metals, rare earth metals, precious metals, tin, aluminum, other Group III and IV metals, And an alloy containing an element. Some typical alloys are LiBi, LiAg, LiIn, LiMg, LiAl, LiMgSi, LiFeSi, LiZr, LiAlCu, LiAlZr, LiAlMg LiB LiCa LiZn LiBi LiNa LiCu LiPt LiCaNa LiAlCuMgZr LiPb LiCaK LiV, LiSn and LiNi. ≪ / RTI > In another embodiment, K, Cs, and Na replace Li, wherein the catalyst is a K atom, a Cs atom, and a NaH molecule.

In another embodiment, the anion may form a hydrogen-type bond with the Li atom of the covalently bonded Li-Li molecule. This hydrogen-type bond can weaken the Li-Li bond to the point where the Li atom acts as a catalytic atom and is present under vacuum energy (to liberate the atom) so that it can form hydrinos. In another embodiment, K, Cs, and Na replace Li, wherein the catalyst is a K atom, a Cs atom, and a NaH molecule.

In one embodiment, the function of the hydrogen dissociation agent is provided by a chemical reaction. H atoms are generated by the reaction of two or more reaction mixture species or by decomposition of one or more species. In one embodiment, Li-Li reacts with LiNH ₂ to form Li atoms, H atoms and Li ₂ NH. Li atoms may also be formed by decomposition or reaction of LiNO ₃ . In another embodiment, K, Cs, and Na replace Li, wherein the catalyst is a K atom, a Cs atom, and a NaH molecule.

In a further embodiment, in addition to a catalyst or a catalyst source for forming low-energy hydrogen, the reaction mixture comprises a heterogeneous catalyst to provide M and H atoms by decomposing MM and MH, such as LiLi and LiH. The heterogeneous catalyst includes at least one member selected from the group consisting of transition elements, noble metals, rare earths and other metals and atoms such as W, Ta, Ni, Pt, Pd, Ti, Al, Fe, Ag, Cr, Cu, Zn, .

In an embodiment of the Li carbon alloy, the reaction mixture contains an excess of Li above the Li-carbon intercalation limit. The excess may range from 1% to 1000%, preferably from 1% to 10%. The carbon may further comprise a hydrogen spillover catalyst having a hydrogen dissociation agent such as Pd or Pt on the activated carbon. In a further embodiment, the cell temperature is higher than the temperature at which Li is fully intercalated into the carbon. The cell temperature may range from about 100 to 2000 캜, preferably from 200 to 800 캜, and most preferably from about 300 to 700 캜. In another embodiment, K, Cs, and Na replace Li, wherein the catalyst is a K atom, a Cs atom, and a NaH molecule.

In an embodiment of the Li silicon alloy, the cell temperature is in the range to release the hydrogen atoms of the silicon alloy, further comprising H. The range may be in the range of about 50 to 1500 占 폚, preferably about 100 to 800 占 폚, and most preferably about 100 to 500 占 폚. The hydrogen pressure may range from about 0.01 to 10 ⁵ Torr, preferably from about 10 to 5000 Torr, and most preferably from about 0.1 to 760 Torr. In another embodiment, K, Cs, and Na replace Li, wherein the catalyst is a K atom, a Cs atom, and a NaH molecule.

The reaction mixture, the alloying compound and the reaction mixture, the alloy and the compound can be added to the catalyst, for example, Li or the catalyst source such as the number of the other element (s), such as the source of other element (s) or compound (s) or other element (s) By mixing it with a paraffin. The catalytic hydride may be LiH, KH, CsH or NaH. The reagents may be mixed by ball milling. The catalyst alloy may also be formed from an alloy source comprising the catalyst and one or more other elements or compounds.

In one embodiment, the reaction mechanism for the Li / N system to form hydrino reactants of Li and H atoms is as follows.

_{LiNH 2 + Li-Li → Li} + H + Li 2 NH (32)

In another embodiment of the Li-Alloy system, the reaction mechanism is similar to that of the Li / N system, where the other element (s) replace N. An exemplary reaction mechanism for carrying out the reaction for forming the hydrino reactants, Li and H atoms, involving a reaction mixture comprising Li and S, Sn, Si and C is as follows.

SH + Li-Li → Li + H + LiS (33)

SnH + Li-Li → Li + H + LiSn (34)

SiH + Li-Li? Li + H + LiSi, and (35)

CH + Li-Li -> Li + H + LiC (36)

A preferred embodiment of the LiS alloy-catalyst system comprises Li with Li ₂ S and Li with LiHS. In another embodiment, K, Cs, and Na replace Li, wherein the catalyst is a K atom, a Cs atom, and a NaH molecule.

Primary Li / N Alloy reaction

In the solid and liquid states, lithium is a metal and the gas contains covalent Li ₂ molecules. To produce the lithium atom, the reaction mixture of the solid fuel comprises a Li / N alloy reactant. The reaction mixture is at least one from the group of Li, LiH, LiNH _2, Li ₂ NH, Li ₃ N, NH _3, dissociation agents, a hydrogen source, for example H ₂ gas or a hydride, a support and a getter for example, LiX (X is a halide) . The dissociation agent is preferably Pt or Pd on a high surface area support which is inert to Li. This may include Pt or Pd on carbon or Pd / Al ₂ O ₃ . The latter support may comprise a protective surface coating of a material such as LiAlO ₂ . Preferred dissociation agents for reaction mixtures comprising Li / N alloys or Na / N alloys are Pt or Pd on Al ₂ O ₃ , Raney nickel (R-Ni) and Pt or Pd on carbon. If the dissociation support is Al ₂ O ₃ , the reactor temperature can be maintained below the temperature that results in a substantial reaction with Li. The temperature may be less than about 250 < 0 > C to about 600 < 0 > C. In another embodiment, Li is in the form of LiH, the reaction mixture is LiNH _2, Li ₂ NH, Li ₃ N, NH _3, dissociation agents, a hydrogen source, for example H ₂ gas or a hydride, a support and a getter for example, LiX (X comprises one or more of the halide), wherein the LiH and Al ₂ O ₃ the reaction is substantially endothermic reaction. In another embodiment, the dissociation agent is unrelated to the balance of the reaction mixture, wherein the dissociation agent passes through the H atoms.

The two preferred embodiments are Al ₂ O ₃ powder on the LiH, LiNH _2, and Pd of the first reaction mixture and which can further comprise a H ₂ gas Al ₂ O ₃ powder, Li, Li ₃ N and hydrogenated Pd on 2 reaction mixture. The first reaction mixture can be regenerated by addition of H ₂ and the second reaction mixture can be regenerated by removing H ₂ and hydrogenating the dissociation agent or reintroducing H ₂ . The regeneration reaction as well as the reaction for regenerating the catalyst and H are shown below.

In one embodiment, LiNH ₂ is added to the reaction mixture. LiNH ₂ produces a Li atom as well as a hydrogen atom according to the following reversible reaction.

Li ₂ + LiNH ₂ → Li + Li ₂ NH + H (37)

Li ₂ + Li ₂ NH → Li + Li ₃ N + H (38)

In one embodiment, the reaction mixture comprises about 2: 1 Li and LiNH ₂ . In the hydrino reaction cycle, Li-Li reacts with LiNH ₂ to form a Li atom, H atom and Li ₂ NH, and the cycle continues according to equation (38). The reactants may be present at any weight percentages.

The mechanism for forming Li ₂ NH from LiNH ₂ involves the first step of forming ammonia [42]:

2LiNH ₂ ? Li ₂ NH + NH ₃ (39)

When LiH is present, it reacts with ammonia to release H ₂ ,

_{* LiH + NH 3 → LiNH 2} + H 2 (40)

The net reaction forms H ₂ with the consumption of LiNH ₂ ,

LiNH ₂ + LiH - > Li ₂ NH + H ₂ (41)

When Li is present, amides are not consumed due to the more energy-efficient reversal of Li and ammonia:

_{Li-Li + NH 3 → LiNH} 2 + H + Li (42)

Thus, in one embodiment, the reactant comprises a mixture of Li and LiNH ₂ to form Li and H atoms according to formulas (37) - (38).

The reaction mixture of Li and LiNH ₂ acting as a Li catalyst and an atomic hydrogen source can be regenerated. During the regeneration cycle, a reaction product mixture comprising species such as Li, Li ₂ NH and Li ₃ N may react with H to form LiH and LiNH ₂ . LiH has a melting point of 688 캜, whereas LiNH ₂ has a melting point at 380 캜, and Li has a melting point at 180 캜. LiNH _2, remove the liquid and any liquid Li is formed at about 380 ℃ physically from LiH and then, by heating the solid LiH independently it can form a Li and H _2. Li and LiNH ₂ may be recombined to regenerate the reaction mixture. And, excess H ₂ from LiH thermal decomposition is reused in the next regeneration cycle, and some supplement H ₂ replaces any H ₂ consumed in the hydrino formation.

In a preferred embodiment, a preferred reaction mixture comprising hydrogenated and non-hydrogenated compounds is formed using competitive reactions in which one reactant is hydrogenated or dehydrogenated to another reactant. For example, by adding hydrogen under appropriate temperature and pressure conditions, the reverse reaction of equations (37) and (38) occurs through a competitive reaction to form LiH such that the hydrogenated product is primarily Li and LiNH ₂ . Alternatively, the reaction mixture comprising the compounds of Li, Li ₂ NH and Li ₃ N groups is hydrogenated to form hydrides and LiH is selected by pumping at the temperature and pressure ranges while achieving selectivity based on differential kinetics. Lt; / RTI >

In one embodiment, Li is deposited as a thin film over a high surface area and a mixture of LiH and LiNH ₂ is formed by the addition of ammonia. The reaction mixture may further contain excess Li. Li and H atoms are formed according to equations (37) and (38), and a state with the energy given by equation (1) is formed in a subsequent reaction. The mixture can then be regenerated by adding H ₂ , followed by heating and pumping, where pumping and removal of H ₂ is optional.

The reversible system of the present invention for producing a lithium catalyst is a Li ₃ N + H system and can be regenerated by pumping. The reaction mixture comprises one or more of Li ₃ N, Li ₃ N sources such as Li and N ₂ , H sources such as H ₂ , hydrogen dissociation agents, LiNH ₂ , Li ₂ NH, LiH, Li, NH ₃ and metal hydrides do. The reaction of H ₂ with Li ₃ N provides LiH and Li ₂ NH while the reaction of Li ₃ N with H from a hydrogen atom source such as H ₂ and a hydride or a hydride undergoing a dissociation reaction is as follows.

Li ₃ N + H? Li ₂ NH + Li (43)

The Li atom catalyst can then react with additional H atoms to form hydrino. Byproducts such as LiH, Li ₂ NH and LiNH ₂ can be converted to Li ₃ N by evacuating the reaction vessel of H ₂ . A typical Li / N-Alloy reaction is as follows:
Li ₃ N + H? Li ₂ NH + Li (44)
Li ₃ N + LiH - > Li ₂ NH + ₂ Li (45)

delete

Li ₂ NH + LiH → Li ₃ N + H ₂ (46)
Li ₂ NH + H? LiNH ₂ + Li (47)
Li ₂ NH + LiH - > LiNH ₂ + ₂ Li (48)
The Li ₃ N, H source and hydrogen dissociation agent are present in any desired molar ratio. Each present in a molar ratio of greater than 0 to less than 100%. Preferably, the molar ratios are similar. In one embodiment, Li ₃ N; LiNH ₂ , Li ₂ NH, LiH, Li, and NH ₃ ; And the molar ratio of the H source, such as the metal hydride, are similar. In another embodiment, K, Cs, and Na replace Li, wherein the catalyst is a K atom, a Cs atom, and a NaH molecule.

In one embodiment, lithium amide and hydrogen react to form ammonia and lithium:

_{1 / 2H 2 + LiNH 2 →} NH 3 + Li (49)

The reaction can induce Li formation by increasing H ₂ concentration. Alternatively, the above-described normal reaction can be induced through the formation of H atoms using a dissociation agent. The reaction by the H atom is given by:

_{H + LiNH 2 → NH 3 +} Li (50)

In embodiments of the reaction mixture comprising at least one compound to form the Li catalyst by reacting with the Li source, said reaction mixture LiNH _2, Li ₂ NH, Li ₃ N, Li, LiH, NH _3, H ₂ and dissociation claim And at least one species from the group. In one embodiment, the Li catalyst is produced from the reaction of LiNH ₂ with hydrogen, preferably a hydrogen atom as given in scheme (50). The ratio of reactants can be any desired amount. Preferably, the ratios are approximate equivalence ratios as in equations (49) and (50). The catalyst formation reaction is reversible with the H source such as H ₂ gas addition reaction which forms a hydrino in place of the reacted gas. The catalytic reaction is given by equations (3) to (5) : ≪ / RTI >

NH ₃ + Li - > LiNH ₂ + H (51)

In another embodiment, K, Cs, and Na replace Li, wherein the catalyst is a K atom, a Cs atom, and a NaH molecule. In a preferred embodiment, the reaction mixture comprises a hydrogen dissociation agent, a hydrogen atom source, and Na or K and NH ₃ . In one embodiment, the ammonia forms an NaNH ₂ or KNH ₂ acting as a catalyst source to react with the Na or K. Another embodiment includes a K catalyst source such as a K metal, a hydrogen source such as NH ₃ , H ₂ and a hydride such as a metal hydride, and a dissociation agent. Preferred hydrides include R-Ni which may act as dissociation agents. Also, hydrinogetters such as KX may be present, where X is preferably a halide such as Cl, Br or I. The cell can be run continuously with replacement of the hydrogen source. The NH ₃ can act as a source of K atoms by reversible formation of KN alloy from KK such as amide, imide or nitrides, or by formation of KH by the emission of K atoms.

In a further embodiment, the reactant comprises a catalyst such as Li and a hydrogen atom source such as H ₂ and a dissociation agent or hydride such as hydrogenated R-Ni. H can react with Li-Li to form LiH and Li, which can also act as a catalyst and react with additional H to form hydrinos. Then, Li can be regenerated by removing H ₂ released from LiH. The plateau temperature at 1 Torr for LiH decomposition is about 560 ° C. LiH can be decomposed at about 500 캜, which is less than the alloy formation and sintering temperature of 0.5 Torr and R-Ni. The molten Li may be separated from the R-Ni, the R-Ni may be hydrogenated again, and the Li and the hydrogenated R-Ni may be recovered in another reaction cycle.

In one embodiment, a Li atom may be deposited on the surface. The surface may be a support or a source of H atoms. The surface may comprise at least one of a hydride and a hydrogen dissociation agent. The surface may be R-Ni which can be hydrogenated. The deposition may be provided from a reservoir containing a Li atom source. The Li source can be controlled by heating. One source that provides Li atoms upon heating is Li metal. The surface can be maintained at a low temperature, such as room temperature, during deposition. The Li-coated surface can be heated to react Li and H to form the H state given by equation (1). Other thin film deposition techniques well known in the art further include embodiments of the present invention. Such embodiments include but are not limited to physical spraying, electrospray, aerosol, electro-arc welding, Knudsen cell controlled release, dispenser-cathode injection, plasma deposition, sputtering and further coating methods and systems, , Electroplating of Li, and chemical vapor deposition of Li. In another embodiment, K, Cs, and Na replace Li, wherein the catalyst is a K atom, a Cs atom, and a NaH molecule.

In the case of Li deposited on the hydride surface, it can be regenerated by removing LiH and Li by heating by pumping, and the hydride can be hydrogenated again by introducing H ₂ , After evacuation, Li atoms can be re-deposited over the regenerated hydride. In another embodiment, K, Cs, and Na replace Li, wherein the catalyst is a K atom, a Cs atom, and a NaH molecule.

Li and R-Ni are present in any desired molar ratio. Each of Li and R-Ni is present in a molar ratio of more than 0 and less than 100%. Preferably, the molar ratios of Li and R-Ni are similar.

In a preferred embodiment, a reaction mixture comprising hydrogenated and non-hydrogenated compounds is achieved using competitive reactions in which one reactant is hydrogenated or dehydrogenated to another reactant. For example, LiH formation is thermodynamically more advantageous than R-Ni hydride formation. However, the LiH formation rate is very low at low temperatures, such as in the range of about 25 DEG C to 100 DEG C, while R-Ni hydride formation takes place at a high rate at a suitable pressure in the range of about 100 Torr to 3000 Torr. Thus, the reaction mixture of Li and hydrogenated R-Ni is pumped at about 400 to 500 DEG C to dehydrogenate LiH, the vessel is cooled to about 25 to 100 DEG C, and hydrogen is added for a period of time to achieve the desired selectivity Can be regenerated from LiH and R-Ni by preferential hydrogenation of R-Ni by addition, followed by evacuation of the cell to remove excess hydrogen. While excess Li is present or added in excess, the R-Ni may be used in a cycle that is repeated by selectively hydrogenating alone. This is accomplished by adding hydrogen in the temperature and pressure range that make up the selective hydrogenation of R-Ni, and then heating the vessel to form H and Li atoms and subsequently removing excess hydrogen before initiating the hydrino reaction . In this process, additional hydride and catalyst sources may be used instead of Li and R-Ni. In a further embodiment, the R-Ni is mostly hydrogenated in a separate manufacturing step using elevated temperature and high pressure hydrogen or using electrolysis. Electrolysis can take place in a basic aqueous solution. The base may be a hydroxide. The counter electrode may be nickel. In this case, R-Ni can provide H atoms for a long period of time by appropriate temperature, pressure, and temperature ramp rates.

LiH has a high melting point of 688 ° C, which may be higher than the temperature at which the dissociation agent is sintered or the dissociation agent metal forms an alloy with the catalyst metal. For example, the LiNi alloy may be formed at temperatures above about 550 [deg.] C when the dissociation agent is R-Ni and the catalyst is Li. Accordingly, it is yet another embodiment, the LiH was converted to LiNH _2, which can be removed at a relatively low melting point can be regenerated to the reaction mixture. The reaction to form lithium amide from lithium hydride and ammonia is as follows:

_{LiH + NH 3 → LiNH 2 +} H 2 (52)

The molten LiNH ₂ can then be recovered at a melting point of 380 ° C. LiNH ₂ can be converted to Li by a decomposition reaction.

In one embodiment involving recovery of molten LiNH ₂ , the gas pressure is applied to the mixture comprising LiNH ₂ to increase its separation rate from the solid components. Separation net or semi-permeable membrane can sustain these solid components. The gas may be an inert gas such as noble gas or nitrogen which limits decomposition of decomposition products such as LiNH ₂ . Molten Li can also be separated using gas pressure. In order to clean any residue from the dissociation agent, a gas flow can be used. An inert gas such as rare gas is preferable. If the residue Li adheres to a dissociation agent such as R-Ni, the residue can be removed by washing with a basic aqueous solution which can also regenerate R-Ni. Alternatively, Li may be hydrogenated to mechanically separate LiH and R-Ni solids and any additional solid compounds present, such as by sieving. In another embodiment, dissociation agents such as R-Ni and other reactants may be physically separated, but hydrogen atoms may be held in close proximity to act on the balance of the reaction mixture. The balance of the reaction mixture and the dissociating agent can, for example, be placed in an open juxtaposed boat. In another embodiment, the reactor further comprises multiple compartments containing the dissociation agent and the balance of the reaction mixture independently. The separation membrane in each compartment allows the hydrogen atoms formed in the dissociation compartment to flow into the balance compartment of the reaction mixture to maintain chemical separation. The separation membrane may be a metal mesh or a semi-permeable inert film which may be metallic. The contents may be mechanically mixed during operation of the reactor. The separate balance of the reaction mixture and its product can be removed and reworked outside the reaction vessel to be recovered independently from the dissociation agent or independently reworked within the reactor.

Other embodiments in which the system produces Li atom catalysts and H atoms include Li, ammonia, and LiH. Li atom catalysts and H atoms can be produced by the reaction of Li ₂ and NH ₃ :

Li ₂ + NH ₃ ? LiNH ₂ + Li + H (53)

LiNH ₂ is the source of NH _{3 in} the following reaction:

₂ LiNH _{2 -} > Li ₂ NH + NH ₃ (54)

In a preferred embodiment, Li is dispersed on a support having a large surface area to react with ammonia. Ammonia also reacts with LiH to produce LiNH ₂ :

_{LiH + NH 3 → LiNH 2 +} H 2 (55)

H ₂ can then react with Li ₂ NH ₃ to regenerate LiNH ₂ :

H ₂ + Li ₂ NH → LiNH ₂ + LiH (56)

In another embodiment, the reactant comprises a mixture of LiNH ₂ and a dissociation agent. The reaction to form a lithium atom is as follows:

LiNH ₂ + H -> Li + NH ₃ (57)

Li may then react with additional H to form a hydrino.

Other embodiments of the Li atom catalyst and system for generating H atoms include Li and LiBH ₄ or NH ₄ X where X is an anion such as a halide. Li atom catalysts and H atoms can be generated by the reaction of Li ₂ and LiBH ₄ :

Li ₂ + LiBH ₄ ? LiBH ₃ + Li + LiH (58)

NH ₄ X can produce LiNH ₂ and H ₂ :

Li ₂ + NH ₄ X? LiX + LiNH ₂ + H ₂ (59)

Then, a Li atom can be produced according to equations (32) and (37). In another embodiment, the reaction mechanism for the Li / N system to form the hydrino reactant of Li atoms with H is as follows:

NH ₄ X + Li-Li → Li + H + NH ₃ + LiX (60)

Wherein X is a counterion, preferably a halide.

Li atom catalysts can be produced by the reaction of H ₂ atoms formed by the dissociation of Li ₂ NH or Li ₃ N and H ₂ :

Li ₂ NH + H LiNH ₂ + Li (61)

Li ₃ N + H? Li ₂ NH + Li (62)

In a further embodiment, the reaction mixture comprises a nitride other than Li, such as Mg, Ca, Sr, Ba, Zn and Th. The reaction mixture may contain a metal which is substituted with Li or forms a metal compound mixed with Li. The metal may be selected from the group of alkali metals, alkaline earth metals and transition metals. The compound may further comprise N, such as amides, imides and nitrides.

In one embodiment, the Li catalyst is chemically produced by an anion exchange reaction such as a halide (X) exchange reaction. For example, at least one of Li metal and Li-Li molecules react with a halide compound to form Li atoms and LiX. Alternatively, LiX reacts with the metal M to form Li atoms and MX. In one embodiment, the lithium metal reacts with a lanthanide element halide to form Li and LiX, wherein X is a halide. One example is that CeBr ₃ and Li ₂ react to form Li and LiBr. In another embodiment, K, Cs, and Na replace Li, wherein the catalyst is a K atom, a Cs atom, and a NaH molecule.

In another embodiment, the reaction mixture further comprises the reagents and products of the Haber process [43]. The product may be NH _x (x = 0, 1, 2, 3, 4). These products can react with Li or a compound containing Li to form Li atoms and H atoms. For example, Li-Li may react with NHx to form Li and possibly H:

_{Li-Li + NH 3 → Li} + LiNH 2 + H (63)

_{Li-Li + NH 2 → LiNH} 2 + Li (64)

_{Li-Li + NH 2 → Li} 2 NH + H (65)

In another embodiment, K, Cs, and Na replace Li, wherein the catalyst is a K atom, a Cs atom, and a NaH molecule.

Mixtures of compounds that melt at a temperature lower than the melting point of one or more individual compounds may be used. Preferably, a eutectic mixture can be formed which is a molten salt mixed with reactants such as Li and LiNH ₂ .

The chemistry of the reaction mixture can vary very substantially depending on the physical state of the reactants and the presence or absence of the solvent or solute or alloyl species added. It is an object of the present invention to change the physical state to control the rate of the reaction and to change the thermodynamics to achieve a sustainable low energy hydrogen reaction by the addition of H from the H source. Li / N alloys systems including reactants such as Li and LiNH ₂ , alkali metals, alkaline earth metals, and mixtures thereof can act as solvents. For example, an excess of Li may include solvated Li and LiNH ₂ reactants that act as a molten solvent for LiNH ₂ , resulting in a relatively different reaction kinetics and thermodynamics than the solid-state mixture. The effect of the electrons, i.e., the control of the low-energy hydrogen reaction dynamics, can be adjusted by controlling the solute and the characteristics of the solvent such as temperature, concentration and molar ratio. The reaction of producing catalyst atoms and hydrogen atoms Next, the latter effect can be used to regenerate the initial reactants. This is a route through which the product can be directly regenerated by the hydrogenation reaction.

One embodiment in which the regeneration of the reactants is facilitated by a solvent or an additive solu- tion or an alloying species comprises a lithium metal wherein the hydrogenation of Li is not complete and Li is present in the solvent and reactants. In a Li solvent, the following regeneration reaction can take place by the addition of H from a source to form LiH:

_{LiH + Li 2 NH → 2Li +} LiNH 2 (66)

In the case of Li / N alloy systems containing reactants such as Li and LiNH ₂ , alkali metals, alkaline earth metals and mixtures thereof can act as solvents. In one embodiment, the solvent is selected to reduce the reaction of LiH to Li and form an unstable solvent hydride with H release. Preferably, the solvent can be one or more of the group of Li (excess), Na, K, Rb, Cs and Ba with corresponding hydrides with low thermal stability while reducing Li < + >. When the melting point of the solvent is higher than desired, as in the case of Ba having a high melting point of 727 DEG C, the solvent is mixed with another solvent such as metal to form a solvent having a relatively low melting point, can do. In one embodiment, one or more alkaline earth metals may be mixed with one or more alkali metals to lower the melting point, increase the Li + reduction potential, and reduce the stability of the corresponding solvent hydride.

Another embodiment wherein the regeneration of the reactants is facilitated by a solvent or an additive solu- tion or alloy species includes potassium metal. The potassium metal in the mixture of LiH and LiNH ₂ can reduce the reaction from LiH to Li and form KH. Since KH is thermally unstable at an intermediate temperature, for example 300 ℃, which can be promoted by adding the hydrogenation reaction to Li and Li in LiNH ₂ NH _2.

Thus, K can catalyze the reaction given by equation (66). The reaction steps are as follows:

LiH + K? Li + KH (67)

_{KH + Li 2 NH → K +} Li + LiNH 2 (68)

Where H is added at a rate at which H is consumed by low energy hydrogen production. Alternatively, K catalytically produces Li and H from LiH, where LiNH ₂ is formed directly from the hydrogenation reaction of Li ₂ NH. The reaction steps are as follows:

Li ₂ NH + 2H → LiH + LiNH ₂ (69)

LiH + K? KH + Li (70)

KH - > K + H (g) (71)

In addition to the desired instability condition of the hydride (KH), amide (KNH ₂ ) is also unstable and the exchange of lithium amide and potassium amide is not thermodynamically favorable. Besides K, Na is also preferred as a metal solvent because it can reduce LiH and has a relatively low vapor pressure. Other examples of suitable metal solvents include Rb, Cs, Mg. Ca, Sr, Ba and Sn. The solvent may comprise a metal mixture, such as a mixture of two or more alkali metals or alkaline earth metals. Preferred solvents are Li (excess) and Na above 380 DEG C because Li is miscible in Na at above this temperature.

In another embodiment, the alkali metal or alkaline earth metal acts as a regeneration catalyst according to equations (70) and (71). In one embodiment, LiNH ₂ is first removed from the LiH / LiNH ₂ mixture by melting the LiNH _2. Subsequently, metal M can be added to catalyze the conversion of LiH to Li. M can be selectively removed by distillation. Na, K, Rb, and Cs form hydrides that decompose at relatively low temperatures and form thermally decomposing amides, and thus in another embodiment, one or more of the compounds of formula (67) to Can act as a reactant for the catalytic conversion of LiH to Li and H according to the corresponding reaction to < RTI ID = 0.0 > K. ≪ / RTI > In addition, some alkaline earth metals such as Sr can form highly stable hydrides and can act to convert LiH to Li by reacting LiH with an alkaline earth metal to form a stable alkaline to hydride. By operating at elevated temperatures, hydrogen can be supplied from the alkaline toto hydride through decomposition by a lithium-containing material present primarily in Li. The reaction mixture may comprise Li, LiNH ₂ , x and dissociation agent wherein X is a lithium compound such as LiH, Li ₂ NH and Li ₃ N, and a small amount of alkali to form a stable hydride to form Li from LiH Have the earth metal. The hydrogen source may be H ₂ gas. The operating temperature should be sufficient to make H available.

In one embodiment, LiNO ₃ can act to produce Li and H source LiNH ₂ in a series of coupling reactions. Consider the embodiment of the catalytic reaction mixture comprising Li, LiNH _2, and LiNO _3. The reaction of Li with LiNH ₂ to form Li ₃ N and release H ₂ is as follows:

LiNH ₂ + ₂ Li → H ₂ + Li ₃ N (72)

The reaction to form water and lithium amide by a balanced H ₂ reduction reaction of the released H ₂ (equation (72)) with LiNO ₃ is as follows:

4H ₂ + LiNO ₃ ? LiNH ₂ + 3H ₂ O (73)

Reaction Scheme 72 can then be run with the resulting LiNH ₂ and the balance Li, and the coupling reaction shown in equations (72) and (73) can occur until Li is completely depleted. The overall reaction is given as:

_{LiNO 3 + 8Li + 3LiNH 2 →} 3H 2 O + 4Li 3 N (74)

Water can be removed by reaction with the getter or kinetically by methods such as condensation to prevent the reaction of the species, such as Li, LiNH _2, Li ₂ NH and Li ₃ N.

Regeneration of exemplary Li catalytic reactants

The present invention also includes a method and system for forming a state given by equation (1) from any by-product formed or regenerated to form a reaction mixture during the reaction. For example, in an embodiment of the energy reactor, the catalytic reaction mixture, for example Li, LiNH _2, and LiNO ₃ is by a method known to the art skilled as given by Cotton (Cotton) and Wilkinson (Wilkinson) [43] It is reproduced from any by-products for example, LiOH and Li ₂ O. The components of the reactant mixture comprising the byproducts may be liquid or solid. The mixture is heated or cooled to the desired temperature and the product is physically separated by means known to those skilled in the art. In one embodiment, the LiOH and Li ₂ O is a solid, Li, LiNH _2, and LiNO ₃ is a liquid, the solid components are separated from the liquid component. LiOH and Li ₂ O can be converted to lithium metal by reduction with H ₂ at high temperature or by electrolysis of molten compounds or mixtures containing them. Among the electrolytic selneun _{LiOH, Li 2 O, LiCl,} KCl, CaCl 2 and NaCl may comprise a molten salt containing one or more. The electrolysis cell is composed of a material resistant to attack by Li, such as a BeO or BN vessel. The Li product can be purified by distillation. LiNH ₂ is formed by means known in the art, for example, by reacting Li with nitrogen and then reducing the hydrogen. Alternatively, LiNH ₂ can be formed directly by the reaction of Li and NH ₃ .

When the initial reaction mixture contains at least one of Li, LiNH ₂ and LiNO ₃ , the Li metal may be regenerated by a method such as electrolysis and LiNO ₃ may be produced from Li metal. One important step in removing the difficult nitrogen fixation step is to react Li metal with N ₂ even at room temperature to form Li ₃ N. Li ₃ N was reacted with H ₂ to form the Li ₂ NH and LiNH _2. Li ₃ N may react with an oxygen source to form LiNO ₃ . In one embodiment, Li ₃ N is lithium (Li), lithium nitride (Li ₃ N), oxygen (O _2), oxygen source, lithium already more than one of the DE (Li ₂ NH) and lithium amide (LiNH ₂₎ Is used in the synthesis of lithium nitrate (LiNO ₃ ) containing reactants or intermediates.

In one embodiment, the oxidation reaction is as follows:

LiNH ₂ + 2O ₂ → LiNO ₃ + H ₂ O (75)

Li ₂ NH + 2O ₂ ? LiNO ₃ + LiOH (76)

Li ₃ N + ₂ O ₂ ? LiNO ₃ + Li ₂ O (77)

Lithium nitrate can be regenerated from Li ₂ O and LiOH using at least one of NO ₂ , NO and O ₂ by the following reaction:

3Li ₂ O + 6NO ₂ + 3 / 2O ₂ ? 6LiNO ₃ (78)

Li ₂ O + 3NO ₂ ? 2LiNO ₃ + NO (79)

NO + 1 / 2O ₂ ? NO ₂ (80)

_{LiOH + NO 2 + NO → 2LiNO} 2 + H 2 O ( industrial process) (81)

₂ LiOH + 2NO ₂ LiNO ₃ + LiNO ₃ + H ₂ O (82)

Lithium oxide can be converted to lithium hydroxide by reaction with steam:

Li ₂ O + H ₂ O → ₂ LiOH (83)

In one embodiment, Li ₂ O is converted to LiOH and then reacts with NO ₂ and NO according to equation (81).

Both lithium oxide and lithium hydroxide can be converted to lithium nitrate by treatment with nitric acid and drying:

Li ₂ O + 2HNO ₃ ? 2LiNO ₃ + H ₂ O (84)

_{LiOH + HNO 3 → LiNO 3 +} H 2 O (85)

LiNO ₃ can be prepared by treating lithium oxide or lithium hydroxide with nitric acid. As suggested by Cotton and Wilkinson, nitric acid can also be produced by known industrial methods such as the Haber process followed by the Ostwald process [43] and subsequently by hydration and oxidation of NO. In one embodiment, an exemplary step sequence is as follows:

_{LiOH + HNO 3 → LiNO 3 +} H 2 O (87)

In particular, the above harbor process can be used to produce NH ₃ from N ₂ and H ₂ at elevated temperature and elevated pressure using a catalyst such as α-iron containing several oxides. Ammonia can be used to form LiNH ₂ from Li. The Oswalt process may be used to oxidize ammonia to NO in a catalyst such as a hot platinum or platinum-rhodium catalyst. The NO may further react with oxygen and water to form nitric acid, which may react with lithium oxide or lithium hydroxide to form lithium nitrate. Crystalline lithium nitrate is then obtained by drying. In another embodiment, NO and NO ₂ react directly with one or more of lithium oxide and lithium hydroxide to form lithium nitrate. The regenerated Li, LiNH ₂ and LiNO ₃ are then recovered in the reactor in the preferred molar ratio.

In a further illustrative of the regeneration, the embodiments of the reactor comprises a reaction product of a Li, LiNH _2, and LiCoO _2. LiOH, Li is the ₂ O, and cobalt (Co), and its low-grade oxide by-products. The reaction can be reproduced by the electrolysis to the LiOH and Li ₂ O Li. LiNH ₂ can be regenerated by the reaction of Li with NH ₃ or N ₂ followed by reaction with H ₂ . CoO ₂ and its lower oxide can be regenerated by reaction with oxygen. LiCoO ₂ can be formed by the reaction of Li and CoO ₂ . Then, Li, LiNH _2, and LiCoO ₂ is recovered from cell batches (batch) or continuous regeneration process. When LiIO ₃ or LiIO ₄ is a reagent for the above mixture, IO ₃ ^- and / or IO ₄ ^- can be regenerated by iodine or iodination reaction with the base and further electrolyzed to the desired anion to form LiIO ₃ or Leached with LiIO ₄ , dried and dehydrated.

NaH molecular catalyst

(여기서, m은 정수임) 중에서 하나가 되도록 하는 연속 에너지 준위로 촉매 시스템을 제공한다.In a further embodiment, a compound comprising hydrogen, such as MH (where H is hydrogen and M is another element), acts as a hydrogen source and a catalyst source. In one embodiment, the sum of the binding energy and the ionization energy of the t electrons by the destruction of the MH bond and the ionization of the t electrons from the M atom is approximately

(Where m is an integer). ≪ / RTI >

One such catalyst system comprises sodium. The binding energy of NaH is 1.9245 eV [44]. The first and second ionization energies of Na are 5.13908 eV and 47.2864 eV, respectively [1]. Based on these energies, the double ionization energy (t = 2) for the binding energy of NaH + Na2 + of Na is 54.35 eV (2 × 27.2 eV) equivalent to m = 2 in equation (2) NaH molecules can act as catalysts and H sources. The catalytic reaction is given by the following formula:

And the overall reaction is as follows:

The hydrogen atom H (1 / p) (p = 1, 2, 3, ... 137) is also given by equation (1), as given in chapter 5 of reference [30] Can be transferred to a low energy state where the transition of one atom is catalyzed by a second atom that resonates and non-radiatively receives m · 27.2 eV while the potential energy is reversed. The overall general expression for the transition of H (1 / p) to H (1 / (p + m)) induced by resonance transfer to H (1 / p ') of 27.2 eV is expressed as:

The transition to H (1/4) (p + m = 4) by H catalyst (p = 1; m = 1) with H (1/3) :

(1/4) ^- > H ₂ (1/4) and H ^- (1/4) + H + ^- > due to the stable binding of H ^- (1/4) in the halide and its ionization stability to other reactive species The H ^- (1/4) formed by the H ₂ (1/4) reaction and the corresponding molecule are preferred products of the hydrogen catalyst.

The sum of the binding energy of NaH, the double ionization energy from Na to Na ²⁺ (t = 2) and the potential energy of H is 81.56 eV (3 · 27.2 eV), which is equivalent to m = 3 in equation (2) , The NaH catalytic reaction can be a harmonious reaction. The catalytic reaction is given as:

And the overall reaction is as follows:

Here, H ⁺ _fast is a fast hydrogen atom with a kinetic energy of 13.6 eV or more.

In one embodiment, the reaction mixture comprises at least one of a NaH molecule and a hydrogen source. The NaH molecule acts as a catalyst to form the H state given by equation (1). The NaH molecular source may comprise one or more of Na metal, a hydrogen source, preferably a hydrogen atom and NaH (s). The hydrogen source may be at least one of H ₂ gas and dissociation agent and hydride. Preferably, the dissociating agent and the hydride may be R-Ni. Preferably, the dissociating agent may also be Pt / Ti, Pt / Al ₂ O ₃ and Pd / Al ₂ O ₃ powder. The solid NaH may be a source of one or more of NaH molecules, H atoms and Na atoms.

In a preferred embodiment, one of the sodium atom and the NaH molecule is provided by the reaction between the molecular form of the metal, ion or Na and one or more other compounds or elements. A source of Na or NaH metal Na, inorganic compounds including Na, for example NaOH, and other suitable Na compound such as NaNH _2, Na ₂ CO ₃ and Na ₂ O (which may be provided in the CRC [41]), NaX ( X May be one or more of halide (s) and NaH (s). The other element may be H, a substituent or a reducing agent. The reaction mixture (1) sodium source for example, Na (m), NaH, NaNH _2, Na ₂ CO _3, Na ₂ O, NaOH, the NaOH doped R-Ni, NaX (X is a halide), and NaX doped R (2) a hydrogen source such as H ₂ gas and dissociation agent and a hydride, (3) a substituent such as an alkali metal or alkaline earth metal, preferably Li, and (4) a reducing agent such as a metal such as an alkali metal, A source of a lanthanide element, a transition metal such as Ti, aluminum, B, a metal alloy such as AlHg, NaPb, NaAl, LiAl and a metal alone or in combination with a reducing agent such as an alkaline earth halide, a transition metal halide, a lanthanide element halide and an aluminum halide And may include one or more. Preferably, the alkali metal reducing agent is Na. Other suitable reducing agents include metal hydrides, for example LiBH _4, NaBH4, LiAlH ₄ or NaAlH _4. Preferably, the reducing agent forms a molecular NaH and Na product e.g. Na, NaH (s), and Na ₂ O by reaction with NaOH. The NaH source may be an R-Ni forming an NaH catalyst, such as an alkali metal or alkaline earth metal, or an Al intermetallic compound of R-Ni, including NaOH and a reactant such as a reducing agent. An exemplary reaction of the added is an alkali metal or alkaline earth metal and an oxidizing agent, for example _{AlX 3, MgX 2, LaX 3} , CeX 3 and TiX _n (where, X is a halide, preferably Br or I Im). The reaction mixture may also include another compound comprising at least one of NaCO ₃ , Na ₃ SO ₄ and Na ₃ PO ₄ which may be doped into a dissociation agent such as a getter or dispersant such as R-Ni. The reaction mixture may further comprise a support, wherein the support may be doped with one or more reactants in the mixture. The support may preferably have a large surface area desirable for the formation of NaH catalyst from the reaction mixture. The support according to the R-Ni, Al, Sn, Al ₂ O ₃ for example, gamma, beta or alpha-alumina, sodium aluminate (cotton [45], a beta-alumina having a different ion, provides a Na ^+, and the ideal the composition Na ₂ O · 11Al ₂ O ₃ having a), Si, silica, silicate, zeolite, lanthanide elements, transition metal, metal alloy such as alkali and alkaline earth alloy, rare earth metals and of Na, SiO ₂ -Al ₂ O ₃ Or Ni supported on SiO ₂ , and other supported metals such as platinum supported on alumina, palladium, or ruthenium. The support has a large surface area, a high-specific surface area (HSA) materials such as R-Ni, zeolite, silicate, aluminate, alumina, alumina nano-particles, the porous Al ₂ O _3, Pt, Ru or Pd / Al ₂ O _3, carbon, it is possible to Pt or Pd / C, the inorganic compounds such as Na ₂ CO _3, silica, and zeolite materials, preferably comprises a Y zeolite powder. In one embodiment, the support (Al ₂ O ₃ support and the presence of the dissociated first if any) such as Al ₂ O ₃ surface is reacted with a reducing agent, such as a lanthanide element - to form a modified support. In one embodiment, the surface Al is substituted with a lanthanide element to form a lanthanide element-substituted support. The support may be doped with a NaH molecular source such as NaOH and reacted with a reducing agent such as a lanthanide element. The subsequent reaction of the lanthanide element-substituted support with the lanthanide element will not substantially change it, and the doped NaOH on the surface can be reduced to the NaH catalyst by reacting with the reducing agent lanthanide element.

In one embodiment in which the reaction mixture comprises an NaH catalyst source, the NaH source may be an Alloy and a hydrogen source of Na. The alloy may be one or more of those known in the art such as an alloy of sodium metal and one or more other alkali or alkaline earth metals, transition metals, Al, Sn, Bi, Ag, In, Pb, Hg, Si, Zr, B, Pt , Pd, or other metal, and the H source may be H ₂ or a hydride.

Reagents such as NaH molecular source, sodium source, NaH source, hydrogen source, substituent and reducing agent are present in any desired molar ratio. Each present in a molar ratio of greater than 0 to less than 100%. Preferably, the molar ratios are similar.

A preferred embodiment comprises a reaction mixture of NaH and Pd on an Al ₂ O ₃ powder, wherein the reaction mixture can be regenerated by addition of H ₂ .

In one embodiment, Na atoms are deposited on the surface. The surface may be a support or H atom source for forming NaH molecules. The surface may comprise at least one of a hydride, and a hydrogen dissociation agent capable of being hydrogenated, such as Pt, Ru or Pd / Al ₂ O ₃ . Preferably, the surface area is large. The deposition may be formed from a reservoir containing a source of Na atoms. The Na source can be controlled by heating. One source that provides Na atoms upon heating is Na metal. The surface can be maintained at a low temperature, such as room temperature, during deposition. The Na-coated surface can be heated to react with Na and H to form NaH, and NaH molecules can be reacted to form the H state given by formula (1). Other thin film deposition techniques known in the art further include embodiments of the present invention. Such embodiments include but are not limited to physical spraying, electro-spraying, aerosol, electro-arc welding, Krusen-cell controlled release, dispenser-cathode injection, plasma deposition, sputtering and further coating methods and systems, Electroplating and chemical vapor deposition of Na. The Na metal is dispersed in a high-surface area material, preferably Na ₂ CO ₃ , carbon, silica, alumina, R-Ni and Pt, Ru or Pd / Al ₂ O ₃ to increase activity, H < / RTI > Other dispersing agents are known in the art, such as cotton [46] et al.

In one embodiment, a reductant or one or more reactants comprising a NaH source such as Na and NaOH undergo an aerosolization reaction to produce and react the corresponding reactant vapor to form an NaH catalyst. Na and NaOH may react in the cell to form an NaH catalyst, where at least one species performs an aerosolization reaction. The aerosolized species may be transferred into the cell and reacted to form a NaH catalyst. The means for carrying the aerosolized species may be a carrier gas. The aerosolization of the reactants can be accomplished using a mechanical stirrer and a carrier gas, such as rare gas, to transport the reactants into the cell to form the NaH catalyst. In one embodiment, the NaH source and Na, which can act as a reactant, are charged and aerosolized by being electrically dispersed. One or more of the reactants, such as Na and NaOH, may be mechanically aerosolized in the carrier gas or may be subjected to ultrasonic aerosolization. The reactant may be passed through an orifice to form a vapor. Alternatively, the reactants may be locally heated to a very high temperature to evaporate or sublimate to form a vapor. The reactant may further comprise a hydrogen source. The hydrogen may react with Na to form an NaH catalyst. Na can be in vapor form. The cell can form a hydrogen atom from H ₂ by including a dissociation agent. Other means of accomplishing the aerosolization known in the art are part of the present invention.

In one embodiment, the reaction mixture comprises at least one species selected from the group consisting of a source of Na or Na sources, a source of NaH or NaH, a source of metal hydrides or metal hydrides, a source of reactants or reactants, A dissociation agent and a hydrogen source. The reaction mixture may further comprise a support. The reactants for forming the metal hydride may include a lanthanide element, preferably La or Gd. In one embodiment, La can react reversibly with NaH to form LaH _n (n = 1, 2, 3). In one embodiment, the hydride exchange reaction forms an NaH catalyst. The reversible general reaction can be given as: < RTI ID = 0.0 >

MaH + M? Na + MH (96)

The reaction given by equation (96) also applies to the other MH-type catalysts provided in Table 2. The reaction is a hydrogen forming process, dissociates to form hydrogen atoms, and can react with Na to form an NaH catalyst. The dissociation agent is preferably at least one of Pt, Pd or Ru / Al ₂ O ₃ powder, Pt / Ti and R-Ni. Preferably, the dissociative support, such as Al ₂ O ₃ , comprises at least one surface where Al is replaced by La or comprises a Pt, Pd or Ru / M ₂ O ₃ powder, where M is a lanthanide element. The dissociation agent may be separated from the remainder of the reaction mixture, wherein the separation membrane passes H atoms.

A preferred embodiment comprises a reaction mixture of NaH, La, and Pd on Al ₂ O ₃ , wherein the reaction mixture comprises, in one embodiment, adding H ₂ and separating NaH and lanthanide element hydride And the lanthanide element hydride is heated to form La and mixed with La and NaH. Alternatively, the regeneration may be performed by melting Na and removing the liquid to separate Na and lanthanide element hydride, heating the lanthanide element hydride to form La, Na being hydrogenated with NaH, mixing La and NaH . The mixing can be performed by ball milling.

In one embodiment, the high-surface area material such as R-Ni may be doped with NaX (X = F, Cl, Br, I). The doped R-Ni reacts with a reagent that displaces the halide and forms one or more of Na and NaH. In one embodiment, the reactants are one or more alkali metals or alkaline earth metals, preferably one or more of K, Rb and Cs. In another embodiment, the reaction product is an alkali or alkaline earth hydride, preferably at least one of KH, RbH, CsH, MgH ₂ and CaH _2. The reactant can be both an alkali metal and an alkaline tosid hydride. The reversible general reaction can be given as: < RTI ID = 0.0 >

NaX + MH- < / RTI > NaH + MX (97)

NaOH catalytic reaction to form NaH catalyst

The reaction from NaOH and Na to Na ₂ O and NaH is as follows:

_{NaOH + 2Na → Na 2 O +} NaH (98)

The exothermic reaction may induce the formation of NaH (g). Thus, the Na metal can act as a reducing agent to form the catalyst NaH (g). Other examples of suitable reducing agent to provide a similarly high pyrogenically reduction reaction with NaH source is an alkali metal, an alkaline earth metal such as Mg and one or more metal halides, for example LiBH of Ca _4, NaBH _4, LiAlH ₄ or NaAlH _4, B, Al , Transition metals such as Ti, lanthanide elements such as La, Sm, Dy, Pr, Tb, Gd and Er, preferably La, Tb and Sm. Preferably, the reaction mixture comprises a high-surface area material (HSA material) having a dopant, such as NaOH, containing an NaH catalyst source. Preferably, the conversion of the dopant to a catalyst having a high surface area is achieved. The conversion can take place by a reduction reaction. The reducing agent may be provided as a gaseous stream. Preferably, Na flows into the reactor as a gaseous stream. In addition to the preferred reducing agent, Na, other preferred reducing agents include other alkali metals, Ti, lanthanide elements or Al. Preferably, the reaction mixture comprises an HSA material, preferably NaOH doped into R-Ni, wherein the reducing agent is Na or intermetallic Al. The reaction mixture may further comprise a source H, for example a hydride, or H ₂ gas and dissociation agents. Preferably, the H source is hydrogenated R-Ni.

In one embodiment, the reaction temperature is maintained below the temperature at which the reducing agent, such as a lanthanide element, forms an alloy with a catalyst source such as R-Ni. In the case of lanthanum, preferably the reaction temperature does not exceed 532 占 폚, which is the alloy temperature of Ni and La, as determined by Gasser and Kefif. Also, the reaction temperature is maintained below a temperature at which the reaction of Al ₂ O ₃ and R-Ni occurs to a considerable extent, such as in the range of 100 ° C to 450 ° C.

In one embodiment, Na ₂ O, formed as a reaction product and giving rise to a NaH catalyst, as given by equation (98), may react with a hydrogen source to form NaOH, which may further serve as an NaH catalyst source. In one embodiment, the regeneration reaction from formula (98) to NaOH in the presence of a hydrogen atom is as follows:

Thus, small amounts of NaOH and Na, and the hydrogen atom source or hydrogen atom act as the catalyst source for the NaH catalyst and, in turn, through multiple cycles of the regeneration reaction as given in equations (98) - (101) . In one embodiment, from the reaction given by equation (102), Al (OH) ₃ can act as a source of NaOH and NaH, where the reaction given by equations (98) To form hydrinos.

In one embodiment, intermetallic Al acts as a reducing agent to form an NaH catalyst. The remainder of the reaction is as follows:

This exothermic reaction can induce the formation of NaH (g), leading to a very exothermic reaction given by Eqs. (88) - (92) wherein NaH regeneration is made from Na in the presence of hydrogen atoms.

Two preferred embodiments include a first reaction mixture of Na and R-Ni containing about 0.5 wt% NaOH (where Na acts as a reducing agent) and a second reaction mixture of R-Ni containing about 0.5 wt% NaOH (Where intermetallic Al acts as a reducing agent). The reaction mixture can be regenerated by adding NaOH and NaH, which can act as a H source and a reducing agent.

In one embodiment of the energy reactor, the NaH source, such as NaOH, is regenerated by the addition of at least one of a hydrogen source such as a hydride and hydrogen gas and a dissociation agent. The hydride and dissociation agent may be hydrogenated R-Ni. In another embodiment, the NaH source such as NaOH doped R-Ni is regenerated by one or more of rehydrogenation, addition of NaH and addition of NaOH, where the addition can be by physical mixing. The mixing can be performed mechanically by means such as ball milling.

In one embodiment, the reaction mixture is also an oxide that forms a very stable oxide and NaH reacts with NaOH or Na ₂ O - further includes a formation reaction. This reaction is cerium, magnesium and lanthanide elements, titanium or aluminum or a compound such as _{AlX 3, MgX 2, LaX 3} , CeX 3 and TiXn (wherein, X is a halide, being preferably Br or I) and for the reduction Compounds such as alkali metals or alkaline earth metals. In one embodiment, the NaH catalyst source comprises R-Ni that includes a sodium compound such as NaOH on its surface. Then, NaOH with an oxide-forming reaction is, for example _{AlX 3, MgX 2, LaX 3} , CeX 3 and TiX _n, and reaction with an alkali metal M are each NaH, MX, and _{Al 2 O 3, MgO, La} 2 O 3, Ce ₂ O ₃ and Ti ₂ O ₃ .

In one embodiment, the reaction mixture comprises NaOH-doped R-Ni, and an alkali or alkaline earth metal added to form at least one of the Na and NaH molecules. Na can react with a source such as H ₂ gas or a hydride such as R-Ni to form a NaH catalyst. Subsequent catalytic reactions of NaH form the H state given by equation (1). The addition of an alkali metal or alkaline earth metal M can reduce Na ^< ^{+ >} to Na by the following reactions:

NaOH + M? MOH + Na (104)

2NaOH + M? M (OH) ₂ + 2Na (105)

M can also react with NaOH to form H and Na:

₂ NaOH + M? Na ₂ O + H ₂ + MO (106)

Na ₂ O + M? M ₂ O + 2Na (107)

The catalyst NaH then reacts with the following reaction:

Na + H- < / RTI > NaH (108)

From the reaction as given in equation (106) by reaction with H and any added H source from R-Ni. Na is a preferred reducing agent because it is an additional source of NaH.

Hydrogen may be added to reduce NaOH and form NaH catalysts:

_{NaOH + H 2 → NaH + H} 2 O (109)

H in R-Ni can reduce NaOH to Na metal and water that can be removed by pumping.

In one embodiment, the reaction mixture comprises at least one compound that reacts with an NaH source to form an NaH catalyst. The source may be NaOH. The compounds may include one or more of the LiNH _2, Li ₂ NH and Li ₃ N. The reaction mixture may further comprise a hydrogen source such as H ₂ . In an embodiment, the reaction of sodium hydroxide and lithium amide to form NaH and lithium hydroxide is as follows:

_{NaOH + LiNH 2 → LiOH + NaH} + 1 / 2N 2 + LiH (110)

The reaction of sodium hydroxide and lithium imide to form NaH and lithium hydroxide is as follows:

_{NaOH + Li 2 OH → Li 2} O + NaH + 1 / 2N 2 + 1 / 2H 2 (111)

The reaction of sodium hydroxide and lithium nitrate to form NaH and lithium oxide is as follows:

_{NaOH + Li 3 N → Li 2} O + NaH + 1 / 2N 2 + Li (112)

Alkali earth hydroxide catalysis to form NaH catalysts

In one embodiment, the H source is provided to the Na source to form the catalytic NaH. The Na source may be a metal. The H source may be a hydroxide. The hydroxide may be at least one of alkali, alkaline earth hydroxide, transition metal hydroxide, and Al (OH) ₃ . In one embodiment, Na reacts with the hydroxide to form its corresponding oxide and NaH catalyst. In embodiments where the hydroxide is Mg (OH) ₂ , the product is MgO. In embodiments where the hydroxide is Ca (OH) ₂ , the product is CaO. Alkaline earth oxides can react with water to regenerate hydroxides as indicated on cotton [48]. Hydroxides can be collected into the precipitate by means such as filtration and centrifugation.

For example, in one embodiment, the NaH catalyst formation reaction and the Mg (OH) ₂ regeneration cycle are given by the following reaction:

_{3Na + Mg (OH) 2 →} 2NaH + MgO + Na 2 O (113)

MgO + H ₂ O? Mg (OH) ₂ (114)

In one embodiment, the NaH catalyst formation reaction and the Ca (OH) ₂ regeneration cycle are given by the following reaction:

_{4Na + Ca (OH) 2 →} 2NaH + CaO + Na 2 O (115)

CaO + H ₂ O → Ca (OH) ₂ (116)

Na / N Alloy Reaction to Form NaH Catalyst

In the solid and liquid states, sodium is a metal and the gas contains shared Na ₂ molecules. To produce an NaH catalyst, the reaction mixture of the solid fuel comprises a Na / N alloy reactant. In one embodiment, the reaction mixture, the solid-fuel reaction and the regeneration reaction, includes those of the Li / N system wherein Na is replaced by Li and the catalyst is the molecule NaH, Molecular NaH rather than H. In one embodiment, the reaction mixture comprises at least one compound that reacts with an NaH source to form an NaH catalyst. The reaction mixture is at least one from the group of Na, NaH, NaNH _2, Na ₂ NH, Na ₃ N, NH _3, dissociation agents, a hydrogen source, for example H ₂ gas or a hydride, a support and a getter for example, NaX (X is a halide) . The dissociation agent is preferably Pt, Ru or Pd / Al ₂ O ₃ powder. For high temperature operation, the dissociating agent may comprise Pt or Pd on a high surface area support that is moderately inert to Na. The dissociation agent may be carbon or Pt or Pd on Pd / Al ₂ O ₃ . The latter support may comprise a protective surface coating of a material such as NaAlO ₂ . The reactants may be present at any weight percentages.

A preferred embodiment comprises a reaction mixture of Na or NaH, NaNH ₂ and Pd on Al ₂ O ₃ , wherein the reaction mixture can be regenerated by addition of H ₂ .

In one embodiment, NaNH ₂ is added to the reaction mixture. NaNH ₂ produces NaH according to the following reversible reaction:

Na ₂ + NaNH _{2 -} > NaH + Na ₂ NH (117)

And

₂ NaH + NaNH ₂ NaH (g) + Na ₂ NH + H ₂ (118)

In the hydrinose reaction cycle, Na-Na and NaNH ₂ react to form NaH molecules and Na ₂ NH 3, and NaH forms hydrinos and Na. Thus, the reaction is reversible according to the following reaction:

Na ₂ NH + H _{2 -} > NaNH ₂ + NaH (119)

And

Na ₂ NH + Na + H? NaNH ₂ + Na ₂ (120)

In one embodiment, NaH in formula (119) is a molecule, so this reaction is another reaction that produces a catalyst.

The reaction of sodium amide and hydrogen to form ammonia and sodium hydride is as follows:

H ₂ + NaNH ₂ → NH ₃ + NaH (121)

In one embodiment, the reaction is reversible. The reaction can be induced to form NaH by increasing H ₂ concentration. Alternatively, the positive reaction can be induced through the formation of H atoms using a dissociation agent. The reaction is given as:

_{2H + NaNH 2 → NH 3 +} NaH (122)

The exothermic reaction can induce the formation of NaH (g).

In one embodiment, the NaH catalyst is produced from the reaction of NaNH ₂ with hydrogen, preferably hydrogen atoms as given in equations (121) and (122). The ratio of reactants can be any desired amount. Preferably, the ratio is an approximate equivalent ratio to that of equations (121) and (122). The reaction for forming the catalyst is reversible by adding a H source, such as H ₂ gas or hydride, to compensate for the reaction, wherein the catalytic reaction is given in equations (88) to (95) Lt; RTI ID = 0.0 > NaH < / RTI >

NH ₃ + Na ₂ → NaNH ₂ + NaH (123)

In one embodiment, the HSA material is doped with NaNH ₂ . The doped HSA material reacts with a reactant that displaces the amide group to form one or more of Na and NaH. In one embodiment, the reactant is an alkali metal or alkaline earth metal, preferably Li. In another embodiment, the reactant is an alkali or alkaline hydrotreated, preferably LiH. The semi-solid may be both an alkali metal and an alkaline tohydrogen. H source, such as H 2 gas, may also be provided in addition to being provided by any other reactants of the reaction mixture, such as hydrides, HSA materials, and replacement reagents.

In one embodiment, sodium amide reacts with lithium to form lithium amide, imide or nitrides and Na or NaH catalysts. The reaction of sodium amide and lithium to form lithium iodide and NaH is as follows:

_{^{2Li + NaNH 2 → Li 2 NH}} + NaH (124)

The reaction of sodium amide and lithium hydride to form lithium amide and NaH is as follows:

_{LiH + NaNH 2 → LiNH 2 +} NaH (125)

The reaction of sodium amide, lithium and hydrogen to form lithium amide with NaH is as follows:

_{Li + 1 / 2H 2 + NaNH} 2 → LiNH 2 + NaH (126)

In one embodiment, the reaction of the mixture forms Na, and the reactant further comprises an H source reacting with Na to form the catalytic NaH by the reaction:

_{Li + NaNH 2 → LiNH 2 +} Na (127)

And

Na + H- < / RTI > NaH (128)

_{LiH + NaNH 2 → LiNH 2 +} NaH (129)

In one embodiment, the reaction is NaNH _2, comprising a reaction product such as alkali metal or alkaline earth metal, preferably Li for replacing an amide of NaNH _2, and further H source e.g. MH (M = Li, Na, K, Rb , Cs, Mg, Ca, Sr and Ba), H ₂ and hydrogen dissociation agents, and hydrides.

Reagent, for example M, MH, NaH, NaNH _2, HSA material, a hydride, and the dissociation of the reaction mixture is present in any desired ratio of the mole of the same. The M, MH, NaNH ₂ and dissociation agents are each present in a molar ratio of more than 0 and less than 100%, preferably the molar ratios are similar.

Other embodiments of the system for producing the molecular catalyst NaH include Na and NaBH ₄ or NH ₄ X where X is an anion such as a halide. Molecular NaH catalysts can be produced by the reaction of Na ₂ and NaBH ₄ :

Na ₂ + NaBH ₄ → NaBH ₃ + Na + NaH (130)

NH ₄ X can produce NaNH ₂ and H ₂ :

Na ₂ + NH ₄ X → NaX + NaNH ₂ + H ₂ (131)

Then, an NaH catalyst may be produced according to the reaction of formulas (117) to (129). In another embodiment, the reaction mechanism for the Na / N system to form the hydrinocatalyst NaH is as follows:

NH ₄ X + Na-Na - > NaH + NH ₃ + NaX (132)

Preparation and regeneration of NH 3 catalyst reactants

In one embodiment, NaH molecules or Na and hydrogenated R-Ni can be regenerated by the system and method after the system and method disclosed for Li-based reactant systems. In one embodiment, Na can be regenerated from solid NaH by evacuating H ₂ released from NaH. The ballast temperature at about 1 Torr for NaH decomposition is about 500 ° C. NaH can be decomposed at about 500 < 0 > C, which is below the alloy formation and sintering temperatures of about 1 Torr and R-Ni. The molten Na can be separated from the R-Ni, the R-Ni can be hydrogenated again, and the Na and the hydrogenated R-Ni can be recovered in another reaction cycle. In the case of Na deposited on the hydride surface, it can be regenerated by removing Na by heating by pumping, and the hydride can be hydrogenated again by introducing H ₂ , and the cell is evacuated in certain embodiments After which Na atoms can be re-deposited over the regenerated hydride.

In a preferred embodiment, a reaction mixture comprising hydrogenated and non-hydrogenated compounds is formed using a competitive reaction in which one reactant is hydrogenated or dehydrogenated to another reactant. For example, the formation of NaH solids is thermodynamically more advantageous than the formation of R-Ni hydrides. However, the formation rate of R-Ni hydride is low at a low temperature, for example, in the range of about 25 DEG C to 100 DEG C, while the R-Ni hydride formation takes place at a high rate at a suitable pressure in the range of about 100 Torr to 3000 Torr. Thus, the reaction mixture of Na and hydrogenated R-Ni is pumped at about 400-500 ° C to dehydrogenate NaH, cool the vessel to about 25-100 ° C, add hydrogen for a period of time to achieve the desired selectivity To hydrogenate the R-Ni preferentially, and then the cell is evacuated to remove excess hydrogen, which can be regenerated from the NaH solids and R-Ni. While excess Na is present or added in excess, the R-Ni may be used in a cycle that is repeated by selective hydrogenation alone. This is accomplished by adding hydrogen in a temperature and pressure range to achieve selective hydrogenation of R-Ni, and then heating the vessel to form H atoms and NaH molecules and subsequent reaction to yield an excess of < RTI ID = 0.0 & ≪ / RTI > Alternatively, a reaction mixture comprising Na and a hydrogen source such as R-Ni may be hydrogenated to form a hydride, and NaH solids may be selectively introduced by pumping in the temperature and pressure ranges while achieving selectivity based on differential kinetics. It can be dehydrogenated.

In one embodiment having a powder reactant, such as a catalyst and a powder source of a reducing agent, the reducing agent powder is mixed with the catalyst source powder. For example, NaOH-doped R-Ni providing an NaH catalyst is each mixed with a metal or metal hydride powder such as a lanthanide element or NaH. In embodiments of the reaction mixture having a HSA material doped or coated with a solid material such as a dissociation agent, a support, or one or more other species in the reaction mixture, the mixing can be accomplished by ball milling or an initial wetting method. In one embodiment, the surface can be coated by impregnating the surface with a solution of a species such as NaOH or NaX (where X is a counter anion, such as a halide) and then drying. Alternatively, the NaOH may be etched by concentrated (deoxygenated) NaOH using the same process [49] as used to etch R-Ni, as is well known in the art, R-Ni. ≪ / RTI > In one embodiment, an HSA material, such as R-Ni doped with a species such as NaOH, reacts with a reducing agent such as Na to form a NaH catalyst that forms a hydrinos. An excess of reducing agent such as Na can then be removed from the product, preferably by evaporation under vacuum at elevated temperature. The reactants can be recycled by condensation. In another embodiment, at least one of the reducing agent and product species is removed using a carrier medium such as a gas or a liquid, such as a solvent, and the removed species is isolated from the carrier medium. The species may be isolated by means well known in the art, such as precipitation, filtration or centrifugation. The species may be recycled directly or may be further reacted to take a chemical form suitable for recycling. In addition, the NaOH can be regenerated by H reduction or by reaction with a water vapor stream. In the case of the former, excess Na can be removed by evaporation, preferably under vacuum, at elevated temperatures. Alternatively, the reaction product can be removed by washing with a suitable solvent such as water, the HSA material can be dried, and the initial reactant can be added. Independently, the product can be recycled to the original reactant by methods known to those skilled in the art. Alternatively, a reaction product such as NaOH separated by R-Ni washing can be used in the process of etching R-Ni to regenerate it. In one embodiment that includes a reactant that is reactive with the HSA material, the product, such as an oxide, may be treated with a solvent such as dilute acid to remove the product. The removed product may then be regenerated by known methods while re-doping and reusing the HSA material.

And as set forth in Cotton [48] the art using the method and system known to the field of those skilled, is a reducing agent for example alkali metal to the corresponding compound, preferably a can be regenerated from the product containing NaOH or Na ₂ O . One method involves electrolysis in a mixture such as a eutectic mixture. In a further embodiment, the reaction product may comprise at least some oxides such as lanthanum elemental metal oxides (e.g. La ₂ O ₃ ). The hydroxide or oxide may be dissolved in a weak acid such as hydrochloric acid to form the corresponding salt, such as NaCl or LaCl ₃ . The gases may be stream streams at low pressure. The salt can be treated with a product reducing agent such as an alkali metal or an alkaline earth metal to form the original reducing agent. In one embodiment, the second reducing agent is an alkaline earth metal, preferably Ca, wherein NaCl or LaCl ₃ is reduced to Na or La metal. Methods known to those skilled in the art are given in Cotton [48], the entire disclosure of which is incorporated herein by reference. Additional CaCl ₃ product is also recovered and recycled. In another embodiment, the oxide is reduced by H ₂ at elevated temperatures.

In one embodiment where NaAlH ₄ is a reducing agent, the product comprises Na and Al that need not be separated from the R-Ni product. R-Ni is regenerated as a catalyst source without separation. Regeneration may be by addition of NaOH. NaOH may be partially dried by dry etching [50] R-Ni Al for reuse. Alternatively, Na and Al are reacted or separated in situ from the reaction product mixture and reacted with H _{2 either} by cotton [51] or as recovered NaH and Al form NaAlH ₄ as shown by the reaction NaAlH ₄ is formed.

R-Ni is the preferred HSA material with NaOH as a source of NaH catalyst. In one embodiment, the Na content obtained from the manufacturer is about 0.01 mg to 100 mg per gram of R-Ni, preferably about 0.1 mg to 10 mg per gram of R-Ni, most preferably about 0.5 to about 10 mg per gram of R-Ni 1 mg to 10 mg. The alloy of R-Ni or Ni may further comprise at least one of a promoter such as Zn, Mo, Fe and Cr. R-Ni or Alloy is W. Al. W. R. Grace Davidson Raney 2400, Raney 2800, Raney 2813, Raney 3201, and Raney 4200, preferably 2400, or an etched or Na-doped embodiment of these materials. The NaOH content of R-Ni can be increased in multiples of about 1.01 to 1000 times. The solid NaOH may be added by mixing by means such as ball milling, or it may be dissolved in the solution to achieve the desired concentration or pH. The solution can be added to R-Ni and water can be evaporated to achieve doping. The doping can range from about 0.1 μg to 100 mg per gram of R-Ni, preferably from about 1 μg to 100 μg per gram of R-Ni, and most preferably from about 5 μg to 50 μg per gram of R-Ni have. In one embodiment, 0.1 grams of NaOH is dissolved in 100 milliliters of distilled water and 10 milliliters of NaOH is added to 500 grams of non-decanted R-Ni (available from W. L. Grace Chemical Company, Lot # 2800/05310 with a total content of about 0.1% by weight). The mixture is then dried. Drying can be achieved by heating to 50 < 0 > C under vacuum for 65 hours. In another embodiment, doping can be accomplished by ball milling about 1-10 mg NaOH per gram of NaOH, such as R-Ni with R-Ni.

R-Ni can be dried according to the standard R-Ni drying process [50]. The R-Ni can be decanted and dried under vacuum at a temperature range of about 10 to 500 占 폚, and is preferably dried at 50 占 폚. The duration may range from about 1 hour to 200 hours, preferably about 65 hours. In one embodiment, the H content of the dried R-Ni is between about 1 ml and 100 ml H / g R-Ni, preferably about 10-50 ml H / g R-Ni wherein the ml gas is in the STP state ) Range. The drying temperature and time, the vacuum pressure, and the flow of gas (if any, such as He, Ar or H ₂ ), during and after drying, are controlled to achieve drying and desirable H content.

In one embodiment of the R-Ni doped with a NaH catalyst source such as NaOH, the production of R-Ni from the Ni / A alloy comprises etching the alloy with an aqueous NaOH solution. The concentration of NaOH, the etching time, and the wash exchange can be varied to achieve a desired level of NaOH incorporation. In one embodiment, the NaOH solution is non-oxygen. The molar concentration is in the range of about 1 to 10 M, preferably in the range of about 5 to 8 M, and most preferably about 7 M. In one embodiment, the alloy is reacted with NaOH at about 50 < 0 > C for about 2 hours. The solution is then diluted with water, such as deionized water, until an Al (OH) ₃ precipitate forms. In this case, the reaction in which NaOH and Al (OH) _{3 form} water-soluble Na [Al (OH) ₄ ] is at least partially prevented so that NaOH is incorporated into R-Ni. The incorporation can be achieved by drying the R-Ni without decanting. The pH of the diluted solution may range from 8 to 14, preferably from 9 to 12, most preferably from about 10 to 11. Argon can be bubbled through the solution for about 12 hours and then the solution can be dried.

Following the reaction in which the reducing agent and the catalyst source form hydrinos (H with the state given by formula (1)), the reducing agent and the catalyst source are regenerated. In one embodiment, the reaction product is separated. The reducing agent product can be separated from the product of the catalyst source. In one embodiment where at least one of the reducing agent and the catalyst source is a powder, the product is mechanically separated based on at least one of particle size, shape, weight, density, magnetic force or dielectric constant. Particles with significant differences in size and shape can be mechanically separated using sieves. Particles with large differences in density can be separated by a buoyancy difference. Particles with large differences in dielectric constant can be electrostatically separated. In one embodiment, the product is pulverized to reverse any sintering action. The pulverization may be performed by a ball mill.

Methods known to those skilled in the art can be applied to the separation of the present invention by the application of routine experimentation. In general, mechanical separation can be separated by settling, centrifugation, filtration and sieving as described in four groups, Earle [52] (the entire disclosure of which is incorporated herein by reference) . In a preferred embodiment, the separation of the particles is achieved by at least one of sieving and use of a mill. The size and shape of the particles can be selected from the starting materials to achieve the desired product separation.

In a further embodiment, the reducing agent is a powder or is converted to a powder and is mechanically separated from other components of the reaction product mixture, such as HSA material. In an embodiment, the Na, NaH, and lanthanide elements comprise at least one of a reducing agent and a reducing agent source, and the HSA material component is R-Ni. The reducing agent product can be separated from the product mixture by converting any unreacted non-powder reducing agent metal to the hydride. The metal hydride may be pulverized to form a powder. The powder can then be separated from that of another product, such as a catalyst source, based on the size difference of the particles. The separation can be performed by agitating the mixture on a series of sieves that select and isolate a particular size range. Alternatively, or in combination with sieving, the R-Ni particles are separated from the metal hydride or metal particles based on the difference in magnetic susceptibility between the particles. The reduced R-Ni product may be magnetic. The unreacted lanthanide elemental metal and the hydrogenated metal and any oxide such as La ₂ O ₃ are each weakly paramagnetic and _half- diamagnetic. The product mixture is agitated in a series of intense magnets alone or in a strong magnet combined with one or more sieves to provide a relatively strong adhesion or adhesion of the R-Ni product particles to the magnets, . In one embodiment where a sieve is used and a magnetic field is applied, the latter adds additional force to gravity to attract smaller R-Ni product particles through the sieve while a weak paramagnetic or a quasi-magnetic property of the reductant product results in a relatively large size So it is kept on the sieve. The alkali metal can be recovered from its corresponding hydride by heating and optionally by applying a vacuum. The hydrogen released can react with the alkali metal in another batch of a repetitive reaction-regeneration cycle. At least one batch may be present in the cycle at various stages. The hydride and any other compound (s) may be separated and then reacted to form a metal separately from the metal formation from the hydride.

In one embodiment, the reaction mixture is preferably regenerated by a deposition technique when the reactant is on the surface of an HSA material such as R-Ni. In a further embodiment having another coated preferred reactant comprising at least one of the NaH catalyst source on the surface and the material supporting the NaH catalyst formation, such as the HSA material, the reactant may be a mixture of an HSA material such as R-Ni . The deposited reagent is Na, NaH, Na ₂ O, NaOH, Al, Ni, NiO, NaAl (OH) _4, β- _{alumina, Na 2 O · nAl 2 O} 3 (n is an integer of 1 to 1000, preferably Is 11), Al (OH) ₃ , and Al ₂ O ₃ in alpha, beta and gamma form. The preferred reactants, or preferred reactants, as well as the order and composition of the gaseous streams and the deposited elements, compounds, intermediates and species which are converted into chemistries and form reactants from the gaseous stream are well known to those skilled in the art of deposition. For example, an alkali metal can be deposited directly, and any metal having a low vapor pressure, such as Al, can be deposited from the gas halide or hydride. Moreover, an oxide product such as Na ₂ O may react with a hydrogen source to form a hydroxide such as NaOH. The hydrogen source may comprise a water vapor stream to regenerate NaOH. Alternatively, NaOH can be formed using an H ₂ or H ₂ source. In addition, hydrogenation of HSA material such as R-Ni can be achieved by supplying hydrogen gas and removing excess hydrogen by such means as pumping. NaOH can be regenerated stoichiometrically by precisely controlling the total number of moles of H reacted from a source such as water vapor or hydrogen gas. Any additional Na or NaH formed in this stage can be removed by evaporation, respectively, and by decomposition and evaporation. Alternatively, the oxide or hydroxide product such as Na ₂ O or excess NaOH may be removed. This can be achieved by conversion to a halide, such as NaI, which can be removed by distillation or evaporation. The evaporation can be achieved by heating and maintaining the vacuum at elevated temperatures. The conversion to the halide can be achieved by reaction with an acid such as HI. The treatment may be performed with a gas stream containing the acid gas. In another embodiment, any excess NaOH is removed by sublimation. This takes place under vacuum at temperatures ranging from 350 to 400 [deg.] C as indicated by cotton [53]. Any evaporation, distillation, transport, gas stream process or associated reactant process may further comprise a carrier gas. The carrier gas may be an inert gas such as rare gas. Additional steps may include mechanical mixing or separation. For example, NaOH and NaH can also be deposited or mechanically removed by methods such as ball milling and sieving, respectively.

If the reducing agent is an element other than the preferred first element such as Na, the other element may be substituted by a second element such as Na using a method known in the art. One step may involve the evaporation of excess reducing agent. High surface area materials such as R-Ni may be etched. The etching can be with a base, preferably NaOH. The etched product can be decanted by virtually any solvent, such as, for example, decanting and possibly water mechanically removed by centrifugation. The etched R-Ni can be dried and recycled under vacuum.

Additional MH-type catalysts and reactions

Another catalyst system of the MH type includes aluminum. The binding energy of AlH is 2.98 eV [44]. The first and second ionization energies of Al are 5.985768 eV and 18.82855 eV, respectively [1]. On the basis of these energies, the AlH molecule has a catalytic activity as the binding energy of AlH ⁺ the double ionization (t = 2) of Al to Al ²⁺ is 27.79 eV (27.2 eV) And H sources. The catalytic reaction is given by:

And the overall reaction is as follows:

In one embodiment, the reaction mixture comprises at least one of an AlH molecule and an AlH molecule source. The AlH molecular source may comprise an Al metal and a hydrogen source, preferably a hydrogen atom. The hydrogen source may be a hydride, preferably R-Ni. In another embodiment, the catalyst AlH is produced by the reaction of a reducing agent with an oxide or hydroxide of Al. The reducing agent comprises at least one of the NaOH reducing agents given above. In one embodiment, the H source is provided to an Al source to form the catalyst AlH. The Al source may be a metal. The H source may be a hydroxide. The hydroxide may be one or more of alkali, alkaline earth hydroxide, transition metal hydroxide and Al (OH) ₃ .

Raney nickel can be prepared by the following two reaction steps:

Na [Al (OH) ₄ ] easily dissolves in concentrated NaOH. It can be rinsed in deoxygenated water. The Ni produced contains Al (about 10% by weight, which can vary), is porous, and has a large surface area. It contains a large amount of H in both the Ni lattice and Ni-AlH _x (x = 1, 2, 3).

The R-Ni reacts with another element to cause the chemical evolution of the AlH molecule, and then proceeds with the catalysis according to the reactions shown in equations (133) to (135). In one embodiment, the AlH release is caused by a reduction reaction, an etch, or an alloy formation. One such other element M is an alkali metal or alkaline earth metal, which reacts with the Ni portion of R-Ni to form AlH _x components, thereby releasing AlH molecules that undergo subsequent catalysis. In one embodiment, M reacts with an Al hydroxide or oxide to form an Al metal, which may also react with H to form AlH. The reaction can be initiated by heating, and the rate can be controlled by controlling the temperature. M (alkali metal or alkaline earth metal) and R-Ni are present in any desired molar ratio. Each M and R-Ni is present in a molar ratio of greater than 0 and less than 100%. Preferably, the molar ratios of M and R-Ni are similar.

In one embodiment, Al atoms are deposited on the surface. The surface may be a support or H atom source for forming AlH molecules. The surface may comprise at least one of a hydride and a hydrogen dissociation agent. The surface may be R-Ni which can be hydrogenated. The deposition may be formed from a reservoir containing a source of Al atoms. The Al source can be controlled by heating. One source that provides Al atoms during heating is Al metal. The surface can be maintained at a low temperature, such as room temperature, during deposition. The Al-coated surface can be heated to react Al and H to form AlH, and AlH molecules can also be reacted to form the H state given by equation (1). Other thin film deposition techniques well known in the art for forming Al and other elements, such as one or more metal layers, further include embodiments of the present invention. Such embodiments include but are not limited to physical spraying, electro-spraying, aerosol, electro-arc welding, Krusen cell controlled release, dispenser-cathode injection, plasma deposition, sputtering and further coating methods and systems, Electroplating and chemical vapor deposition of Al.

In one embodiment, the AlH source comprises at least one of R-Ni and other Raney metals or alloys such as Ni, Cu, Si, Fe, Ru, Co, Pd, Pt and other elements of Al known in the art R-Ni or an alloy. The R-Ni and alloys may also include one or more of the cocatalysts such as Zn, Mo, Fe and Cr. R-Ni or Alloy is W. Al. Grace Raney 2400, Raney 2800, Raney 2813, Raney 3201, Raney 4200, or an etched or Na-doped embodiment of these materials. In another embodiment of the AlH catalyst system, the catalyst source comprises a Ni / Al alloy wherein the Al to Ni ratio is about 10-90%, preferably about 10-50%, more preferably about 10-30 %. The catalyst source may comprise palladium or platinum and further comprises Al as the Raney metal.

AlH source may further include AlH _3. AlH ₃ can be deposited on or in conjunction with Ni to form a NiAlH _x alloy. The alloy may be activated by the addition of a metal such as an alkali metal or an alkaline earth metal. In one embodiment, the reaction mixture comprises AlH _3, R-Ni and metals such as alkali metals. The metal may be supplied by gravity from a source that flows from the reservoir to evaporation or from R-Ni at elevated temperatures. In one embodiment, the AlH molecule or Al and the hydrogenated R-Ni can be regenerated by a system and method subsequent to the system and method disclosed for other reactant systems. Another catalyst system of the MH type comprises chlorine. The binding energy of HCl is 4.4703 eV [44]. The first, second and third ionization energies of Cl are 12.96764 eV, 23.814 eV and 39.61 eV, respectively [1]. On the basis of these energies, HCl was found to be the highest value since the triple ionization (t = 3) of Cl to Cl ³⁺ of HCl + 80.86 eV (3 · 27.2 eV) Catalyst and H source. The catalytic reaction is given by:

And the overall reaction is as follows:

In one embodiment, the reaction mixture comprises an HCl or HCl source. The source can be NH ₄ Cl or a solid acid and a chlorine such as an alkali or alkaline earth chloride. The solid acid may be one or more of MHSO ₄ , MHCO ₃ , MH ₂ PO ₄ and MHPO ₄ , where M is a cation such as an alkali or alkaline earth cation. Other such solid acids are known to those skilled in the art. In one embodiment, the reactant comprises an HCl catalyst in an ionic lattice such as an alkali or alkaline earth halide, preferably HCl in a chloride. In one embodiment, the reaction mixture comprises a strong acid such as H ₂ SO ₄ and an ionic compound such as NaCl. The reaction of an acid with an ionic compound such as NaCl produces HCl in the crystal lattice and acts as a hydrinocatalyst and H source.

Generally, a hydrino produced by the breakdown of the MH bond at a continuous energy level such that the sum of the binding energy and the ionization energy of the t electrons is approximately m 27.2 eV, where m is the number given in Table 2 The MH type hydrogen catalyst and the ionization of each of the t electrons from the respective M atoms are given in Table 2 below. Each MH catalyst is presented in the first column and the corresponding MH binding energy is presented in the second column. The atom M of the MH species presented in the first column is ionized to provide a net reaction enthalpy of m · 27.2 eV with the binding energy of the second column. The enthalpy of the catalyst is shown in column 8, where m is given in column 9. Electrons participating in ionization are presented as ionization potentials (also called ionization energy or bond energy). For example, the binding energy of NaH, 1.9245 eV [44], is presented in the second column. The ionization potential of the nth electron of an atom or ion is denoted by IP _{n and} is given in CRC [1]. For example, Na + 5.13908 eV → Na ⁺ + e- and Na + 47.2864 eV → Na ²⁺ + e ^- . The first ionization potential, IP ₁ = 5.13908 eV, and the second ionization potential, IP ₂ = 47.2864, are shown in the second and third columns, respectively. The net reaction enthalpy for destruction of the NaH bond and the double ionization of Na are 54.35 eV as shown in the eighth column and m = 2 as shown in the ninth column. Also, H reacts with each of the MH molecules shown in Table 2 below to form a hydrin with a quantum number p that increases by 1 relative to the catalytic reaction product of MH alone, as shown in the exemplary equation (92) (Equation (1)).

Table 2 below shows MH type hydrogen catalysts capable of providing a net reaction enthalpy of about m · 27.2 eV.

In another embodiment of the MH-type catalyst, the reactant comprises a source of SbH, SiH, SnH and InH. In an embodiment providing the catalyst MH, the source comprises at least one of M, H ₂ and MH _x sources such as Sb, Si, Sn and In and H ₂ sources and SbH ₃ , SiH ₄ , SnH ₄ and InH ₃ .

The reaction mixture further comprises an H source and a catalyst source, wherein H and at least one source of the catalyst may be a solid acid or NH ₄ X, wherein X is a halide, preferably Cl, to form an HCl catalyst. Preferably, the reaction mixture may include a NH ₄ X, a solid acid, NaX, LiX, KX, NaH, LiH, KH, Na, Li, K, a support, a hydrogen dissociation one or more of the claim and H _2, Wherein X is a halide, preferably Cl. Wherein the solid acid is selected from the group consisting of NaHSO ₄ , KHSO ₄ , LiHSO ₄ , NaHCO ₃ , KHCO ₃ , LiHCO ₃ , Na ₂ HPO ₄ , K ₂ HPO ₄ , Li ₂ HPO ₄ , NaH ₂ PO ₄ , KH ₂ PO ₄ and LiH ₂ PO ₄ Lt; / RTI > The catalyst may be one or more of NaH, Li, K and HCl. The reaction mixture may further comprise at least one of a dissociation agent and a support.

Other thin film deposition techniques well known in the art further include embodiments of the present invention. Such an embodiment may be applied to a variety of coating processes and systems such as physical spray, electrospray, aerosol, electric arc welding, Krusen cell controlled release, dispenser-cathode injection, plasma deposition, sputtering and further coating methods and systems, Electroplating and chemical vapor deposition of M, wherein MH comprises a catalyst.

In the case of an MH source including M alloys, such as AlH and Al, respectively, the alloy may be hydrogenated by an H ₂ source such as H ₂ gas. H ₂ may be fed to the alloy during the reaction, or H ₂ may be fed to form the desired H content of Alloy with varying H pressure during the reaction. In this case, the initial H ₂ pressure may be about zero. The alloy may be activated by the addition of a metal such as an alkali metal or an alkaline earth metal. For MH catalysts and MH sources, the hydrogen gas may be maintained at a range from about 1 Torr to 100 atm, preferably from about 100 Torr to 10 atm, and more preferably from about 500 Torr to 2 atm. In another embodiment, the hydrogen source is provided from a hydride such as an alkali metal or alkaline earth metal hydride or a transition metal hydride.

High-density hydrogen atoms undergo a three-body-collision reaction to form hydrino, where two H atoms are ionized, one H atom transitions to a state given by Eq. (1) . The reaction is given as:

And the overall reaction is as follows:

In another embodiment, the reaction is given as:

And the overall reaction is as follows:

In one embodiment, the material providing the high density of H atoms is R-Ni. H atom is from the R-Ni within the decomposition H and H ₂ H ₂ gas supply source, for example provided in the cell can be provided from one or more of the dissociation of H _2. The R-Ni reacts with an alkali metal or an alkaline earth metal M to accelerate the formation of the H atom layer, thereby causing a catalytic action. The R-Ni can be regenerated by evaporating the metal M and then re-hydrogenating the R-Ni by adding hydrogen.

references

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41. D. R. Lide, CRC Handbook of Chemistry and Physics, 86th Edition, CRC Press, Taylor & Francis, Boca Raton, (2005-6), pp. 4-45 to 4-97 which is hereby incorporated by reference.

42. W. I. F. David, M. O. Jones, D. H. Gregory, C. M. Jewell, S. R. Johnson, A. Walton, P. Edwards, "A Mechanism for Non-stoichiometry in the Lithium Amide / Lithium Imide Hydrogen Storage Reaction," J. Am. Chem. Soc., 129, (2007), 1594-1601.

43. F. A. Cotton, G. Wilkinson, Advanced Organic Chemistry, Interscience Publishers, New York, (1972).

44. D. R. Lide, CRC Handbook of Chemistry and Physics, 86th Edition, CRC Press, Taylor & Francis, Boca Raton, (2005-6), pp. 9-54 to 9-59.

45. F. A. Cotton, G. Wilkinson, C. A. Murillo, M. Bochmann, Advanced Inorganic Chemistry, Sixth Edition, John Wiley & Sons, Inc., New York, (1999), Chp 6.

46. F. A. Cotton, G. Wilkinson, C. A. Murillo, M. Bochmann, Advanced Inorganic Chemistry, Sixth Edition, John Wiley & Sons, Inc., New York, (1999), p. 95.

47. J-G. Gasser, B. Kefif, " Electrical resistivity of liquid nickel-lanthanum and nickel-cerium alloys ", Physical Review B, Vol. 41, No. 5, (1990), pp. 2776-2783.

48. F. A. Cotton, G. Wilkinson, C. A. Murillo, M. Bochmann, Advanced Inorganic Chemistry, Sixth Edition, John Wiley & Sons, Inc., New York, (1999).

49. V. R. Choudhary, S. K. Chaudhari, " Leaching of Raney Ni-Al alloy with alkali, kinetics of hydrogen evolution ", J. Chem. Tech. Biotech, Vol. 33a, (1983), pp. 339-349.

50. R. R. Cavanagh, R. D. Kelley, J. J. Rush, " Neutron vibrational spectroscopy of hydrogen and deuterium on Raney Nickel ", J. Chem. Phys., Vol. 77 (3), (1982), pp. 1540-1547.

51. F. A. Cotton, G. Wilkinson, C. A. Murillo, M. Bochmann, Advanced Inorganic Chemistry, Sixth Edition, John Wiley & Sons, Inc., New York, (1999), pp. 190-191.

52. R.L. Earle, M.D. Earle, Unit Operations in Food Processing, The New Zealand Institute of Food Science & Technology (Inc.), Web Edition 2004, available at http://www.nzifst.org.nz/unitoperations/.

53. F. A. Cotton, G. Wilkinson, C. A. Murillo, M. Bochmann, Advanced Inorganic Chemistry, Sixth Edition, John Wiley & Sons, Inc., New York, (1999), p. 98.

Experiment

The number of equations, the number of sections, and the number of references given later in this Experimental Section refer to those described in the experimental section of the disclosure of the invention.

summary

(p ≤ 137 는 정수임) 는 수소 여기 상태에 대해 리드베리 방정식에서 공지된 파라미터 n = 정수를 대신함) 이다. 리튬 원자 및 NaH 분자는 촉매로서 사용되기 때문에, 촉매 기준에 부합한다 - 수소 원자의 포텐셜 에너지, 27.2 eV 의 정수 배수 m (예, Li 에 대해서는 m = 3 및 NaH 에 대해서는 m = 2) 와 같은 엔탈피 변화를 갖는 화학적 또는 물리적 공정. 신규 알칼리 할리도 하이드리노(hydrino) 수소화물 화합물 (MH*X; M = Li 또는 Na,×= 할라이드) 및 디하이드리노 분자 H₂(1/4) 의 상응하는 하이드리노(hydrino) 수소화물 이온 H^-(1/4) 의 에너지 준위의 폐쇄형 방정식에 기반을 둔 구체적인 예상을, 화학적으로 발생된 촉매작용 반응물을 사용하여 테스트했다.The data from a broad spectrum of survey techniques shows firmly and consistently that hydrogen can exist at a lower energy state than previously thought. The expected reaction involves the non-emissive resonance energy transfer from other stable hydrogen atoms to the energy-accepting catalyst. The product is a fraction of the hydrogen atom called H (1 / p), " hydrino atom " in the Rydberg state,

(p < 137 is an integer) is substituted for the parameter n = integer known in the Reed-Berry equation for the hydrogen excited state). Since the lithium atom and the NaH molecule are used as catalysts, they meet the catalyst criteria - the enthalpy, such as the potential energy of the hydrogen atom, an integer multiple of 27.2 eV (e.g., m = 3 for Li and m = Chemical or physical process with change. The corresponding hydrino hydride ion of the novel alkali halide hydrino hydride compound (MH * X; M = Li or Na, x = halide) and the dihydrino molecule H ₂ (1/4) Specific predictions based on a closed equation of H ^- (1/4) energy level were tested using chemically generated catalytic reactants.

) 및 약 1-2 V/cm 의 아주 낮은 필드(field) 강도에서 공명 전달, 즉 rt-플라즈마로 불리는 플라즈마의 형성의 관찰이었다. H Balmer α 라인의 시간 의존성 라인 넓어짐(증대)이 아주 빠른 H (>40 eV) 에 대응하여 관찰되었다.First, the Li catalyst was tested. Li and LiNH ₂ were used as a source of lithium atoms and atomic hydrogen. Using the flow batch calorimetry, the measured power from 1 g Li, 0.5 g LiNH ₂ , 10 g LiBr, and 15 g Pd / Al ₂ O ₃ was about 160 W with an energy balance of ΔH = -19.1 kJ. The observed energy balance was 4.4 times the maximum theoretical based on known chemistry. Next, Raney nickel (R-Ni) is used as a dissociation agent when the power reaction mixture is used in chemical synthesis, where LiBr not only captures H ₂ (1/4) in the crystal but also forms LiH * X Which served as a getter of the catalytic product H (1/4). ToF-SIMs showed a LiH * X peak. 1H MAS NMR LiH * Br and LiH * I showed large and pronounced high field resonance at about -2.5 ppm, corresponding to H ^- (1/4) in the LiX matrix. NMR peaks was consistent with the interstitial H ₂ (1/4), and the rotational frequency of the 4 _² H ² (1/4) times of the conventional H ₂ at 1.13 ppm were observed at 1989 cm-1 in the FTIR spectrum . The XPS spectrum recorded for the LiH * Br crystal shows peaks at about 9.5 eV and 12.3 eV, which can not be assigned to any known element based on the absence of other primary element peaks, but the H ^- (1/4) bond energy. A further signature of the energy process is that when Li atoms are present with hydrogen atoms,

) And the formation of a plasma called resonance transmission, rt-plasma, at a very low field strength of about 1-2 V / cm. The time dependence of the H Balmer α line was observed in response to a very rapid H (> 40 eV) line expansion (increase).

NaH uniquely achieves kinetics because the catalytic reaction depends on the release of the intrinsic H, which forms H (1/3), which reacts further to form H (1/4) We suffer incidental transmission of danger. High temperature differential scanning calorimetry (DSC) was performed on ionic NaH under a helium atmosphere at a very slow temperature gradient (0.1 ° C / min) to increase the amount of molecular NaH formation. The new heating effect of -177 kJ / mole NaH was observed in the temperature range of 640 ℃ - 825 ℃. To achieve high power, R-Ni with a surface area of about 100 m ₂ / g is surface-coated with NaOH and reacts with Na metal to form NaH. Using the flow-flow calorimetry, the measured power from 15 g of R-Ni was found to be less than that of the R-Ni starting material, R-NiAl alloy when reacted with Na metal, of ΔH = -36 kJ With an energy balance of about 0.5 kW. The observed energy balance of the NaH reaction was -1.6 × 104 kJ / mole H ₂ , -241.8 kJ / mole H ₂ More than 66 times the combustion enthalpy.

ToF-SIMs showed a sodium hydrino hydride, NaH _x , peak. The 1H MAS NMR spectra of NaH * Br and NaH * Cl showed a large and distinct high field resonance at -3.6 ppm and -4 ppm, respectively, corresponding to H ^- (1/4), and the NMR peak at 1.1 ppm showed H ₂ / 4). NaH * Cl from the reaction of solid acid KHSO ₄ , the sole source of NaCl and hydrogen, contained two fractional hydrogen states. The H ^- (1/4) NMR peak was observed at -3.97 ppm and the H ^- (1/3) peak was also present at -3.15 ppm. The corresponding H ₂ (1/4) and H ₂ (1/3) peaks were observed at 1.15 ppm and 1.7 ppm, respectively. XPS spectrum recorded for the pools NaH LiH * * Br Br and is at about 9.5 eV and 12.3 eV consistent with the results from the KH * I H ^- showed the (1/4) peak, on the other hand, sodium hydro Reno (hydrino ) hydride is H at 6 eV in the absence of halide ^peak-I showed the two states with a hydrogen fraction in addition to (1/3) XPS peak. The expected rotational transmission with an energy of 4 ² times the normal H ₂ was also observed from the excited H ₂ (1/4) using a 12.5 keV electron beam.

I. Introduction

Mills [1-12] interpreted the structure of the combined electrons using classical principles, and subsequently, with the result of observing the fundamental phenomena of physics and chemistry from quark scale to cosmos, the Grand Unified We have developed a single theory based on a principle called Theory of Classical Physics (GUTCP). This paper is in two series, first with two specific predictions of GUTCP that polishes the presence of low energy states of hydrogen atoms, indicating a robust new energy source and the transfer of hydrogen atoms to low energy states [2 ].

The GUTCP predicts a reaction involving non-emissive resonant energy transfer from another stable hydrogen atom to an energy-accepting catalyst to form hydrogen at a lower energy state than previously thought possible. Specifically, the product is a hydrogen atom in the form of H (1 / p), the fractional Ridberg state of a hydrogen atom termed a " hydrino atom " Replacing the known parameter n = integer in the Berry equation). Since it is expected that He ⁺ , Ar ⁺ , Sr ⁺ , Li, K, and NaH are expected to be used as catalysts, it meets the criteria of the catalyst - chemical or physical, with enthalpy changes such as the potential energy of a hydrogen atom, an integer multiple of 27.2 eV fair. Data from a broad spectrum of illumination techniques firmly and consistently supports these states, termed hydrino, and the presence of the corresponding diatomic molecule, called the dihydrino molecule, for " small hydrogen ". Some of these previous related studies supporting the possibility of novel reactions of hydrogen atoms generating hydrogen in fractional quantum states that are lower energy than the conventional " ground " (n = 1) state include Extreme Ultraviolet (EUV) spectroscopy , Characteristic emissions from catalysts and hydride ion products, low-energy hydrogen emissions, chemically-formed plasma, Balmer alpha line amplification, H line inversion distribution, high electron temperature, anomalous plasma afterimage duration, [13-40].

Recently, there was some unexpected announcement of astronomical physical results that supported the existence of Hydro North. In 1995, Mills published GUTCP estimates [41] that the cosmic expansion is accelerating from the same equation that accurately predicted the mass of the top quark before it was measured. Surprisingly, this was confirmed until 2000. Mills made other predictions about the nature of the dark matter based on the almost identifiable GUTCP. Based on recent evidence, Bournaud et al. [42-43] suggested that dark matter is a dense molecular form of hydrogen that behaves differently than it can by unobservable except by gravity effects. The theoretical model predicted that dwarfism formed from the collisional debris of a massive galaxy should be free of nonbaryonic dark matter. As such, his gravity must match the stars and the gas within the star. Analyzing the observed gas kinetics of such a recirculating galaxy, Bournaud et al. [42-43] reported that the gravitational mass of a series of dwarf galaxies lying in a ring around a massive galaxy, . Contrary to the predictions of the cold dark matter (CDM) theory, the results demonstrate that it contains a large mass of dark components, which is calculated to be about twice the visible matter. Although this baryonic dark matter is claimed to be a cold hydrogen molecule, it is distinct from conventional hydrogen molecules in that it is not tracked at all by conventional methods such as the release of CO lines. These results are consistent with the prediction that dark matter is a dihydrino molecule.

The emission lines recorded on the cold interstellar zone containing dark matter corresponded to the fractional Rydberg state of the hydrogen atom given by H (1 / p), equations (2a) and (2c) [29]. Such a discharge line with energies of q 13.6 eV where q = 1, 2, 3, 4, 6, 7, 8, 9, or 11 is also responsible for the microwave discharge of helium with 2% (EUV) spectroscopy [27-29]. The reason for these chemical and physical processes to have enthalpy changes such as He ⁺ is an integer multiple of 27.2 eV on a catalyst basis is ionization at 54.417 eV, 2 · 27.2 eV. The product of the He ⁺ catalysis, H (1/3), can also be used as a catalyst to transition to another state H (1 / p).

J. R. Reidberg has shown that all spectral lines of hydrogen atoms are given by a complete empirical relationship:

(1)

(One)

(Where R = 109,671 cm-1, n _f = 1,2,3, ..., n _j = 2, 3, 4, ..., and n _i > n _f ). Bohr, Schroedinger, and Heisenberg have developed a theory of hydrogen atoms, each providing energy levels according to the Rydberg equation.

(2a)

(2a)

n = 1, 2, 3, (2b)

(Where, e is the elementary charge, ε _o is the dielectric constant of a vacuum, a _H is the radius being a hydrogen atom). The excited energy state of a hydrogen atom is given by equation (2a) for n> 1 in equation (2b). The n = 1 state is a "ground" state for a "pure" photon (ie, the n = 1 state can absorb a photon and can go into an excited state but can not emit a photon, Can not go to state). However, electron transition from ground state to low energy state may be possible by resonant non-emissive energy transfer, such as multipole coupling or resonant collision mechanism. Processes such as hydrogen molecule bond formation that occur without photons and require collision are common [44]. In addition, some commercially available phosphors are based on resonant non-emissive energy shearing involving multipole coupling [45].

Previous theoretical as reported in [1, 13-40], the hydrogen atom is any atom, excimer, ions and two potential energy of the hydrogen storage (hydrogen atom, _h E = 27.2 eV (wherein, E _h is one with tri ( Hartree)) to the reaction of the gaseous effluent to the reactor. It is necessary that the specific species (e.g., He ⁺ , Ar ⁺ , Sr ⁺ , K, Li, HCl, and NaH) that can be identified based on known electron energy levels are present with the hydrogen atom . The reaction is characterized by an extremely hot excited state H [13-17, 19-20, 32-39], and non-emissive energy transfer to form hydrogen atoms with lower energies than unreacted hydrogen atoms corresponding to the fractional number of electrons, Followed by q 13.6 eV emission or q 13.6 eV transmission to H. In other words,

(2c)

(2c)

Replaces the known parameter n = integer in the Rydberg equation for the hydrogen excited state. The n-1 state of hydrogen and n = 1 / integer state of hydrogen are non-emissive, but the transition between two non-emissive states with n = 1 to n = 1/2 is possible through non-emissive energy transfer Do. Thus, the catalyst provides a net positive enthalpy of the reaction of m · 27.2 eV (ie, this catalyst resonantly allows non-emissive energy transfer from hydrogen atoms, emits energy around, Affecting electron transfer). As a result of the non-emissive energy transfer, the hydrogen atoms become unstable and release additional energy until a low energy non-emissive state with the main energy levels according to equations (2a) and (2c) is achieved.

The catalytic product, H (1 / p), may react with electrons to form a new hydride ion H ^- (1 / p) with binding energy E _B [1, 13-14, 18, 30].

(여기서, mp 는 양성자의 질량임) 로 표시되는 환산 전자 질량, a_o 는 Bohr(보어) 반경이고, 이온 반경은

이다. 방정식 (3)으로부터, 수소 이온의 계산된 이온화는 0.75418 eV 이고, 리케(Lykke) [46] 에 의해 주어진 실험값은 6082.99 ± 0.15 cm^-1 (0.75418 eV)이다.Where h is the plaque constant bar, μ _o is the permeability of the vacuum, m _e is the mass of the electron and μ _e is the mass of the electron,

(Where mp is the mass of the proton), a _o is the Bohr (bore) radius, and the ion radius is

to be. From equation (3), the calculated ionization of the hydrogen ion is 0.75418 eV and the experimental value given by Lykke [46] is 6082.99 +/- 0.15 cm ^-1 (0.75418 eV).

The upper field shifted NMR peak is a direct evidence of the presence of low energy state hydrogen with a reduced radius for normal hydrogen ions and an increase in semiconductive shielding of protons. The migration is given by the sum of the normal hydride ion H ^- and components due to the low energy state [1, 15]:

(4)

(4)

Here, H ^- and p = 0 for a, H ^-, and p = an integer> 1, for the (1 / p), is the fine structure constant.

H (1 / p) can react with a proton and two H (1 / p) can react to form H ₂ (1 / p) ⁺ and H ₂ (1 / p) respectively. Hydrogen molecular ion and molecular charge and current density functions, coupling distances, and energies have been described from Laplacian in ellipsoidal coordinates with suppression of non-emission [1, 6].

The total energy E _T of the hydrogen molecule ion having the center field of + pe at each focal point of the elongated ellipsoidal molecular orbital is:

Where p is an integer, c is the speed of light in vacuum, μ is the converted core mass, and k is the harmonic load constant previously described in a closed equation with only a fundamental constant [1, 6]. The total energy of the hydrogen molecule having the center field of + pe at each focal point of the elongated ellipsoidal molecular orbital is:

The bond dissociation energy of the hydrogen molecule H ₂ (1 / p), E _D is the difference between the corresponding energy of the corresponding hydrogen atom and E _T :

E _D = E (2 H (1 / p)) - E _T (8)

Here, in [47]

E (2H (1 / p) ) = -p 2 27.20eV (9)

E _D is given by the equations (8-9) and (7):

Calculation and measurement parameters of H ₂ , D ₂ , H ⁺ ₂ , and D ⁺ ₂ from Reference [1, 6] are given in Table 3 below.

[1, 6]은 H₂ 와 H₂(1/p)에 대한 p = 정수 > 1 에 의존하는 용어의 이동의 합에 의해 주어진다:The 1H NMR resonance of H ₂ (1 / p) is expected to be the upper field from the resonance of H ₂ due to the fractional radius in elliptical coordinates [1, 6], where the electrons are very close to the nucleus. The expected migration to the previously derived H ₂ (1 / p)

[1, 6] is given by the sum of the translations of terms dependent on p = integer> 1 for H ₂ and H ₂ (1 / p):

Here, p = 0 for H ₂ .

E _vib is the molecular vibration energy for the transition from υ = 0 to υ = 1 of the small H ₂ (1 / p), [1, 6].

E _vib = p ² 0.55902 eV (13)

Where p is an integer and the experimental vibrational energy for the transition from v = 0 to v = 1 is given by Beutler [48] and Hertzberg [49].

The rotation energy E _rot for the J to J + 1 transition of the small H ₂ (1 / p) is [1, 6].

Where p is an integer and I is the moment of inertia and the experimental rotational energy for the J = 0 to J = 1 transition of H ₂ is given by Atkins [50].

The p ² dependence of the rotational energy results from the inter-nucleus distance to the moment of inertia I and the inverse p dependence of the corresponding impulse. The expected core-to-nucleus distance 2c 'for H ₂ (1 / p) is:

(15)

(15)

The formation of a new state of hydrogen is very vigorous. A new source of chemically generated or enhanced plasma, which is based on the new resonant energy transfer mechanism (rt-plasma) and can be a new power source, has been developed. One such source operates by heating the hydrogen dissociation agent and catalyst to an incandescent lamp to provide hydrogen atoms and a gaseous catalyst, respectively, so that the catalyst reacts with hydrogen atoms to produce a plasma. Surprisingly, it has been found that strong EUV emissions can be obtained from hydrogen atoms that simply or variably ionize at the potential energy of the hydrogen atom, an integer multiple of 27.2 eV, and surprisingly low field strengths of about 1-2 V / cm from any atomizing element or gas phase ion But also by Mills et al. [13-21, 38-39] at low temperatures (eg, 10 ³ K).

K ~ K ³⁺ provides a net enthalpy corresponding to three times the potential of the hydrogen atom in the reaction. It has previously been reported that the presence of these gaseous atoms with thermal dissociation hydrogen formed rt-plasma with strong EUV emission with normal inverse Lyman density [13-21, 38-39]. Other non-catalytic metals, such as Mg, do not produce plasma. Significant line augmentation of the Balmer alpha, beta and gamma lines of 18 eV was observed. The emission from the rt-plasma occurred even when the electric field applied to the plasma was zero. Since there is no conventional discharge power source, the formation of plasma requires a vigorous reaction. The cause of Doppler line width increase is the relative thermal motion of the emitter relative to the observer. The linewidth increase is a measure of the atomic temperature and a significant increase was expected and observed for K [13-21, 38-39] as well as for catalyst, Sr ⁺ or Ar ⁺ , with hydrogen. Observations of high hydrogen temperatures without the prior art indicate that the rt-plasma should have a source of free energy. More vigorous chemical reactions were related to the fact that the increase was time-dependent [13-14, 20]. Thus, the thermal power balance was measured in calories. Since the reaction is exothermic, an excess power of 20 mW cm ^-3 was measured by Calvet calorimetry [20]. In a further experiment, KNO ₃ and Raney nickel were used as sources of K catalyst and atomic hydrogen, respectively, resulting in a corresponding exothermic reaction. Energy balance, combustion of hydrogen, by assuming the maximum possible H ₂ list [14], the oxygen in the 300-fold ΔH = -17,925 kcal / KNO ₃ mole, and the atmosphere of what is expected for the most vigorous known chemistry of KNO ₃ in a greater than 60 times the maximum enthalpy of a family of -57.8 kcal / mole H ₂ group it was _{ΔH = -3585 kcal / mole H 2} . Substantial evidence of more vigorous the reaction catalyst is very stable novel hydride ions and molecules H ^- to involve resonance energy transfer between hydrogen atoms and K to form the (1/4), and H ₂ (1/4), each of the , [13-15, 24-26, 30-31]. Characteristic emissions were observed from K ³⁺ confirming resonance-free emission energy transfer of 3 · 27.2 eV from the hydrogen atom used as the catalyst expected. From equation (3), the binding energy E _B of H ^- (1/4) is:

The product hydride ion H ^- (1/4) was observed by EUV spectroscopy at 110 nm corresponding to the expected binding energy of 11.2 eV [13-15, 24-26, 30-31]. The identity of H ^- (1/4) was previously confirmed by XPS measurement of its binding energy. By having additional features at 8.9 eV and 10.8 eV, the XPS spectrum of KH * I, which is different from KI, does not correspond to any other primary element peaks and has H ^- (1/4) E _b = 11.2 eV in two different chemical environments It was a match. The ¹ H MAS NMR spectrum of the new compound KH * Cl for external tetramethylsilane (TMS) showed a large and distinct high field resonance at -4.4 ppm, corresponding to an absolute resonance shift of -35.9 ppm, consistent with the theoretical prediction of p = (13-15, 25-26, 30-31). Elemental analysis confirmed these compounds containing alkali metals, halogens and hydrogen, and the non-known hydride compounds of this composition could be found in the literature with high field transfer hydride NMR peaks. Conventional alkali hydrides alone or mixed with alkali halides showed subfield migration peaks [13-15, 25-26, 30-31]. From this document, a list of alternatives of H ^- (1 / p) as a possible source of high field NMR NMR peaks was defined as H at the center of kJ. This was removed by the absence of a strong and distinctive infrared oscillation band at 530 cm ^-1 due to the substitution of Cl ^- with H ^- in KCl [51].

As a further feature, H ^- is (1/4) * KH FTIR analysis of this crystal I was carried out, the equation (14), the interstitial H ₂ (1/4) with a given energy by the expected rotation by was observed. Rotating lines were observed at 145-300 nm from the atmospheric pressure electron beam excited argon-hydrogen plasma [13-14]. An unprecedented energy interval of 4 ² times the hydrogen was established at a quarter of the H ₂ distance, and confirmed the H ₂ (1/4) (equation (13-15)). The spectrum was asymmetric with the P branch dominant corresponding to the absence of dense rotational state in the excited v = 1 oscillatory state. This was due to the high rotational energy (10 times the thermal energy), the short lifetime of the rotational excited state and the low cross-sectional area of the electron beam rotational excitation, while vibrational dipole excitation was permitted. Thus, only the υ = 1, J = O state is fairly dense from the electron beam excitation, and the transition occurs with AJ> 0 during the transition from v = 1 to v = 0. The KH * Cl with H ^- (1/4) by NMR was incidental to the 12.5 keV electron beam and the beam emitted a similar emission of interstitial H ₂ (1/4) as observed in an argon-hydrogen plasma [13-14]. In particular, H ₂ (1/4) captured in the lattice of KH * Cl can be detected by using a 12.5 keV electron gun at a pressure below which a gas can generate a detectable emission (<10 ^-5 Torr) Electron beam excitation was investigated by windowless EUV spectroscopy. The rotational energy of H ₂ (1/4) was similarly confirmed by this technique. As a result of these efforts, it is expected that the results of intense hydrogen Lyman emission, normal Lyman density, excessive persistence of persistence, very strong hydrogen atom, characteristic alkali-ion release due to catalysis, anticipated new spectral lines, From the plasma formed by the vigorous hydrino formation reaction with power measurements beyond any conventional chemistry [13-40] that matched the catalytic reaction of atomic hydrogen to form the lino ion designation H ^- (1 / p) . Since the comparison of the ion and experimental energy is a direct proof of low-energy hydrogen with a large exotherm that is unclear during the formation of hydrogen, we report the results when these experiments are repeated with the further expected Li and NaH catalysts.

Catalyst systems that make, use and analyze expected hydride compounds carry lithium atoms. The primary and secondary ionization energies of lithium are 5.39172 eV and 75.64018 eV, respectively [52]. At that time, the doubly ionized (t - 2) reaction of Li - Li ²⁺ has a net enthalpy of reaction of 81.0319 eV, corresponding to 3 · 27.2 eV.

And, the total reaction is

Lithium is a solid and liquid metal, the gas is a covalent Li ₂ molecule [53], each with a binding energy of 110.4 kJ / mole [54]. To yield a lithium atom, LiNH ₂ was added to the reaction mixture. LiNH ₂ also yields a hydrogen atom according to the reverse reaction [55-64]:

Li ₂ + LiNH ₂ → Li + Li ₂ NH + H (20)

* And

Li ₂ + Li ₂ NH → Li + Li ₃ N + H (21)

The reaction energy of lithium amide to lithium nitrides and lithium hydrides is an invention [65-66]:

_{4Li + LiNH 2 → Li 3 N} + 2LiH ΔH = -198.5 kJ / mole LiNH 2 (22)

Therefore, the reaction must take place to a considerable extent. Specific predictions of the vigorous response given by equation (17-19) were tested by rt-plasma formation and H line amplification. The developed electric power was measured by flow-flow calorimetry. Then, equations (3) and H each having a given energy by the ^(5-15) of the expected product (1/4), and H ₂ (1/4) are each solid-state magic proton nuclear magnetic resonance spectroscopy (MAS ¹ F NMR), X-ray photoelectron spectroscopy (XPS), time-of-flight secondary ion mass spectrometry (ToF-SIMs), and Fourier transform infrared spectroscopy (FTIR).

A compound containing hydrogen, such as MH (where M is other than hydrogen), is used as a source of hydrogen and a source of catalyst. The catalytic reaction is provided by breakdown of the M - H bond + ionization of the t electrons from each atom M to the continuous energy level so that the sum of the binding energy and ionization energy of t electrons is about m · 27.2 eV, M is an integer). One such catalyst system involves sodium. The combined energy NaH is 1.9245 eV [54] and the primary and secondary ionization energies of Na are 5.13908 eV and 47.2864 eV, respectively [52]. Based on these energies, the NaH molecule is used as a catalyst and H source because the binding energy of the double ionization (t = 2) of the binding energy NaH Na - Na ^{2 +} is 54.35 eV (2 · 27.2 eV). The catalytic reaction is given by:

And the overall reaction is as follows:

The hydrogen atom H (1 / p) p = 1, 2, 3, ... 137 is given by the equations (2a) and (2c), as given in chapter 5 and reference [29] Where the transition of one atom is facilitated by another that accepts m · 27.2 eV as a resonant non-emissive with incidental opposite changes in the potential energy. The overall general equation for the transition from H (1 / p) to H (l / (p + m)) induced by resonance transfer from m · 27.2 eV to H (1 / p '

In the case of high hydrogen atom concentration, the transition from H (1/3) (p = 3) to H (1/4) (p + m = 4) by H as catalyst (p = 1; Can be accelerated:

The reason why the NaH catalytic reaction can be matched is that the sum of the binding energy NaH, the double ionization of Na - Na ²⁺ (t = 2), and the potential energy of H is 81.56 eV (3 · 27.2 eV).

And the overall reaction is as follows:

Where H ⁺ _fast is a fast hydrogen atom with kinetic energy of at least 13.6 eV. H ^- (1/4) forms a stable Hala Ido hydride, the reaction the reaction _{2H (1/4) → H 2 (} 1/4) , and ^{H - (1/4) + H +} → H 2 (1 / 4) with the corresponding molecule [13-15, 24-26, 30-31]. The corresponding hydrino atom H (1/4) is the preferred end product consistent with the observation that the p = 4 quantum state has a higher polarity than the quadrupole giving a long theoretical lifetime. H (1/4) can be formed directly from H (e.g., equations (36-38)) or through multiple transitions (e.g., equations (23-27)). In the latter case, the quantum number p = 2 corresponding to the dipole and quadrupole transition, respectively; l = 0 and p = 3; High-energy H (Mp) states with l = 0,1,2 have theoretically acceptable fast transitions.

Sodium hydrides are generally in the form of ionic crystalline compounds formed by the reaction of gaseous hydrogen with sodium metal. Also, in the gaseous state, sodium contains covalent Na ₂ molecules with a binding energy of 74.8048 kJ / mole [53]. When NaH (s) is heated at a very slow temperature gradient (0.1 ° C / min) under helium atmosphere to form NaH (g), the expected exothermic reaction given by equation (23-25) DSC). &Lt; / RTI &gt; To achieve high power, the chemical system was designed to greatly increase the amount and rate of formation of NaH (g). The reaction of NaOH and Na to Na ₂ O and NaH (s) calculated from the forming heat [54, 65] releases ΔH = -44.7 kJ / mole NaOH:

NaOH ( ₂ ) NaH2O + NaH (s) DELTA H = -44.7 kJ / mole NaOH (31)

This exothermic reaction could form NaH (g) and was used for its exothermic reaction given by Equation (23-25). The regeneration reaction in the presence of a hydrogen atom is as follows:

_{Na 2 O + H → NaOH +} Na ΔH = -11.6 kJ / mole NaOH (32)

NaH → Na + H (1/3) ΔH = -10,500 kJ / mole H (33)

And

NaH → Na + H (1/4) ΔH = -19,700 kJ / mole H (34)

Thus, small amounts of NaOH, Na, and hydrogen atoms are used as catalyst sources for NaH catalysts which in turn form hydrin in a large yield of hydrinos through multiple cycles of the regeneration reaction, such as those given by equations (31-34). R-Ni, which has a high surface area of about 100 m ² / g and contains H, was coated with NaOH and reacted with Na metal to form NaH (g). Since the energy balance in the formation of NaH (g) is negligible due to the associated small amount, the energy and power due to the hydrino reaction given by equation (23-25) can be clearly determined . The R-Ni 2400 was then hardlocked with about 0.5 wt% NaOH, and the intermetallic Al was used as the reactant to form the NaH catalyst during the calorimetry. The reaction of NaOH + Al - Al ₂ O ₃ + NaH calculated from the formation heat [65] is exothermic by ΔH = -189.1 kJ / mole NaOH. The balance reaction is given by:

_{3NaOH + 2Al → Al 2 O 3} + 3NaH ΔH = -189.1 kJ l mole NaOH (35)

This exothermic reaction can form NaH (g) and is used for its exothermic reaction given by Equation (23-25), where the regeneration of NaH occurs from Na in the presence of hydrogen atoms. For 0.5 wt% NaOH, the exothermic reaction given by equation (35) provided a myriad of ΔH = -0.024 kJ background heat during the measurement.

It has been reported in [28-29] that the reaction product H (1 / p) may undergo further reaction to a low energy state. For example, the catalytic reaction of Ar ⁺ -Ar ²⁺ forms H (1/2), which is further used as both catalyst and reactant to form H (1/4) [1, 13-14, 28-29] And the corresponding preferred molecule H ₂ (1/4), which is observed with different catalysts [13-14]. Thus, the reference H has a given energy respectively, by reference [29] Equations (23-25) and the product equation (3) and (5-15) of NaH estimated catalyst from Table 1 ^(1/3) and H ₂ (1/4). The product was tested by MAS &lt; 1 &gt; H NMR and ToF-SIMs.

Other catalyst systems of type MH involve chlorine. The binding energy of HCl is 4.4703 eV [54]. The primary, secondary, and tertiary ionization energies of Cl are 12.96764 eV, 23.814 eV, and 39.61 eV, respectively [52]. Based on these energies, HCl can be used as catalyst and H source because the triple ionization (t = 3) of the binding energy of HCl + Cl to Cl ³⁺ is 80.86 eV (3.227.2 eV). The catalytic reaction is given by:

Cl ³⁺ + 3e ^- + H ^- &gt; HCl + 80.86 eV (37)

And the overall reaction is as follows:

At that time, the expected product is H ₂ (1/4).

Alkali chlorides contain both Cl and H from common H ₂ O contaminants. Thus, any HCl may be formed in the crystalline matrix in an interstitial form. Since H ⁺ is the easiest substituent to Li ⁺ and substitution is likely to occur in Cs ⁺ , the alkali chloride forms HCl that undergoes catalytic action, resulting in the formation of H ₂ 1/4). Due to the difference in lattice structure, MgCl ₂ can not form an HCl catalyst; Therefore, it is used as a chlorine control. This condition applies to halides of copper which can be used as controls for the formation of other alkaline earth halides and transition metal halides such as H ₂ (1/4). One exception from this set is Mg ²⁺ in the proper lattice because the ionization of Mg ²⁺ - Mg ³⁺ is approximately 3.227.2 eV, 80.1437 eV [52]. This hypothesis is based on the assumption that an alkali halide, MgX ₂ (X = F, Cl, Br, I), with the objective of determining whether the expected release of H ₂ ), and electron beams for CuX _{2 (X = F, Cl,} Br) - this was tested by emission spectroscopy. NMR was recorded for the parent compounds to find the corresponding expected H ₂ (1/4) peak to be compared with the emission results.

II. Experimental Method

Rt-Plasma and Line Widening Method. LiNH ₂ argon-hydrogen (95/5%) and LiNH ₂ hydrogen rt-plasma were produced in the above-described experimental apparatus [15-21] (FIG. 1), which was equipped with a gas inlet and outlet passage Includes thermally insulated stainless steel cells with plugs. Titanium filaments (55 cm length, 0.5 mm diameter) were used as heaters and hydrogen dissociation devices in the cell. 1 g of LiNH ₂ (Alfa Aesar, 99.95%) was placed in the center of the cell in a glove box under 1 atm of argon. The cell was sealed and taken out from the glove box. The cell was flowed at a pressure of 1 Torr at a rate of 30 sccm while maintaining the cell at 50 캜 for 4 hours. The filament power was increased by 20 W every 20 minutes to reach 200 W. At 120 W, the filament temperature was estimated to be in the range of 800-1000 ° C. The outer wall temperature of the cell was about 700 ° C. Thereafter, the cell was operated without flowing or flowing the argon-hydrogen (95/5%) maintained at 1 Torr in the cell at a rate of 5.5 sccm. Further, the cell was operated while flowing hydrogen gas instead of argon-hydrogen (95/5%). LiNH ₂ was evaporated using a filament heater to demonstrate the presence of Li-line. The presence of argon-hydrogen or the presence of hydrogen plasma was determined by recording in the visible spectrum in the Balmer region and for this the CCD detector [15- 21] (Jobin Yvon Horiba 1250 M) was used. The width of the 656.3 nm Ballmer family line emitted from the hydrogen-LiNH ₂ rt-plasma with argon-hydrogen (95/5%) -LiNH ₂ or titanium filament was measured initially and periodically during testing. As a control, each of the above experiments was carried out by flowing a gas containing LiNH ₂ .

Differential scanning calorimetry (DSC). Differential scanning calorimetry (DSC) measurements were performed using the DSC mode of a calorimeter (HT-1000, Setaram, France). Two alumina globes were used in the sample compartment and the reference compartment, respectively. The two gloves allowed the atmospheric reaction to be controlled. 0.067 g of NaH was placed in a flat-bottom Al-23 crucible (Alfa-Aesar, 15 mm height x 10 mm outer diameter x 8 mm inner diameter). The crucible was then placed on the bottom of the sample group alumina globe cell. As a reference group, an aluminum oxide sample (Alfa-Aesar, -400 mesh powder, 99.9%) was charged in the same kind of Al-23 crucible with the same mass as the sample group. All samples were handled in a glove box. Each alumina globe cell was sealed in a glove box, removed from the glove box, and quickly attached to the calorimeter. They were immediately decompressed to a pressure of 1 mTorr or less. The cell was refilled with 1 atm of helium, re-depressurized, and then refilled with 760 Torr of helium. The cells were then placed in an oven and their locations were fixed in the DSC equipment. The temperature of the oven was adjusted to the desired starting temperature of 100 ° C. The temperature of the oven was raised from 100 ° C to 750 ° C at a rate of 0.1 ° C / min. As a control, MgH ₂ was used instead of NaH. An MgH ₂ sample (Alfa-Aesar, 90%, residual Mg) was added to the sample cell and aluminum oxide (Alfa-Aesar) of the same mass was added to the reference cell. All samples were handled in a glove box.

Water - flow rate, batch calorimeter. A cylindrical stainless steel reactor with a volume of about 60 cm3 (outer diameter 1.0 ", length 5.0", and outer wall thickness 0.065 ") is shown in Figure 2. The cell has an internally welded cylindrical thermocouple with a length of 2.5" and an outer wall thickness of 0.035 " , And a thermocouple (Type K, Omega) read by a meter (DAS). For a cell sealed with a hot valve, an outer diameter welded to the end, 1/4 " (I) 1 g of Li, 0.5 g of LiNH ₂ , 10 g of LiBr and 15 g of Pd / Al ₂ O ₃ , (ii) a solution of Na (Iii) 15 g of NaOH-doped R-Ni, and (iv) 3 wt% Al (OH) ₃ -doped Ni / Al alloy. When the passageway was sealed by spot welding, a tube having an outer diameter of 1/4 "and an outer wall thickness of 0.02" SS was used. The reaction was loaded in a glove box, the valve was attached to the passage tube to seal the cell, the cell was taken out of the glove box and connected to the vacuum pump. The cells were shrunk by depressurization to a pressure of 10 mTorr. Thereafter, the cell was sealed with a valve or the remaining tube was sealed and sealed with a 1/2 "spot welding.

The reactor was installed in the cylindrical calorimeter chamber shown in Fig. The stainless steel chamber had an inner diameter of 15.2 cm, an outer wall thickness of 0.305 cm, and a length of 40.4. Both ends of the chamber were sealed using a removable stainless steel plate and a Viton ™ o-ring (o-ring). The space between the reactor and the inner wall of the cylindrical chamber was filled with a high temperature insulator. The gas composition and pressure in the chamber were controlled by controlling the thermal conductivity between the reactor and the chamber. The interior of the chamber was filled first with 1000 Torr of helium to allow the cell to reach room temperature and then the cell temperature was increased by reducing the pressure during calorimetry. Then, 1000 Torr of helium was added to increase the thermal conductivity from the hot cell to the cooling water and to control the heat change associated with the pressure-volume change. The relative dimensions of the reactor and chamber were adjusted so that the heat flowing from the reactor to the chamber was primarily radial. The chamber was cooled using fast flowing cooling water through a 6.35 mm ID copper tube tightly wound about 63 times on the outer cylindrical surface of the chamber. The reactor and chamber were designed to safely absorb a 50 kW thermal power pulse for 1 minute. The absorbed energy was released sequentially to the cooling water flow according to the prescribed method for calorimetric measurement. The temperature rise of the cooling water was measured at the inlet and outlet of the cooling coil using a precision thermistor probe (Omega, OL-703-PP, 0.01 ° C). The temperature of the water at the inlet was controlled by a constant temperature water bath (Cole Parmer, digital Polystat, model 12101-41) with a temperature stability of 0.01 C and a cooling capacity of 900 W at 20 캜. In order to reduce the temperature fluctuation caused by circulation in the water tank, an insulated 8 liter capacity tank was installed only in the lower part of the water tank. Coolant flow in the equipment was maintained by an FMI model QD variable flow positive displacement experiment pump. The cooling water flow rate was controlled by a high resolution variable area flowmeter. The flowmeter was calibrated by its own flow screening. Secondary flow measurements were performed by a turbine flowmeter (McMillan, G111 Flometer, 1%) that continually fed the flow rate to the data acquisition device. The calorimeter chamber was installed in a sealed HDPE tank filled with a melamine foam insulator to minimize the heat loss rate of the device. It can be seen that the heat loss rate is 2 to 3% when compared with the measured input power by precisely measuring the thermal power emission to the cooling water.

The calorimeter is adjusted by a precision heater operating during the adjustment time to determine the percentage recovery of the total energy added by the heater. The energy recovery rate was calculated by integrating the total output power P _T during that time. The power was calculated by the following equation.

(39)*

(39)

Wherein R is the total flow rate, C _p is the specific heat of water, is the absolute value of the difference in temperature between the inlet and the outlet where, two thermistors were corrected for differences in the case of flow constant, the input power. As a first step in the calibration test, a hollow reaction cell (identical to the power cell containing the reactant to be tested next) was depressurized to less than 1 Torr and inserted into the calorimeter vacuum chamber. The chamber was depressurized and filled with helium to reach 1000 Torr. Unpowered devices reached equilibrium after approximately two hours, which is the time at which the temperature difference between the thermistors becomes constant. The device was run for one more hour to obtain a difference value according to the correction values of the two sensors. The degree of correction was 0.036 &lt; 0 &gt; C, and the corrected values were constant when viewing the data collected during the entire test run.

To increase the temperature of the cell per input power, the helium in the chamber was evacuated through a vacuum pump during the last 10 minutes of the equilibration time of 10 hours, and the chamber was maintained at a pressure of less than 1 Torr by continuous pumping operation. A power of 100.00 W was supplied to the heaters (50.23 V and 1.991 A) for 50 minutes. During this time, the cell temperature increased to approximately 650 ° C and the maximum value of the water temperature difference (water temperature difference between the outlet and inlet) was approximately 1.2 ° C. After 50 minutes, the power indicated zero. To increase the heat transfer rate to the cooling water, the chamber was repressurized to 100 Torr of helium and the device was allowed to reach full equilibrium after 24 hours as confirmed by equilibrium observation in a flow thermistor.

The hydrolysis reaction followed the procedure for calibration, but the cell contained the sample. The equilibration time in the chamber using 1000 Torr helium was 90 minutes. A power of 100.00 W was supplied to the heater, and after 10 minutes, the helium was discharged from the chamber. The cell was heated faster than the exit rate and at 57 minutes the reagent was allowed to reach a limit temperature of 190 DEG C, the hydrinot reaction. The start of the reaction was confirmed as the cell temperature rapidly increased to about 378 ° C in about 58 minutes. After 10 minutes, the power was turned off and helium was slowly injected into the cell at a rate of 150 sccm for 1 hour.

0.1 wt% NaOH-doped R-Ni 2800 or 0.5 wt% NaOH-doped R-Ni 2400 as the reactant (elemental analysis was performed by WR Grace Davidson, the manufacturer, wt% NaOH, (1 g) and LiNH ₂ (0.5 g), LiBr (10 g) (Alfa Aesar, ACS grade 99 +%), and Pd / Al _The products obtained from the reaction of the reaction mixture containing ₂ O ₃ (15 g) (1% Pd, Alfa Aesar) were analyzed and analyzed using a closed sample holder (Bruker, Model # A100B37 Ray diffraction analysis (XRD) using a diffractometer (XRD) using Cu radiation with a power of 40 kV / 30 mA over a range of 10 ° to 70 ° with a step interval of 0.02 ° and a calculation time of 8 hours Siemens, D5000). Also, in a 16.5 cc stainless steel cell connected to a vacuum unit with a total volume of 291 cc, weighing samples of R-Ni were heated from 25 ° C to 550 ° C to decompose into physically adsorbed or chemisorbed gases and released The gas was identified and measured. Mass spectrometer, quantitative gas chromatography (HP 5890 Series II - microfilled column (length 2 m, outer diameter 1/16 ", ShinCarbon, ST 100/120), N ₂ carrier gas (flow rate 14 ml / min) 80 ° C, detector temperature 100 ° C, and thermal conductivity detection temperature 100 ° C), and the measured pressure, volume, and temperature were substituted into the ideal gas equation to derive the hydrogen content. Hydrogen was most dominant in each analysis using water and less than 2% of methane was measured by gas chromatography. Trace amounts of water in the R-Ni and the control were each measured with hydrogen, Was performed by liquefying H ₂ O in liquid nitrogen trap, withdrawing hydrogen, and evaporating water using 0.5 g of sample to the extent that it did not increase to saturated water-vapor pressure at room temperature.

Synthesis of LiH * Br, LiH * I, NaH * Cl and NaH * Br and Solid Phase ¹ H MAS NMR. As additional reactants, lithium bromo and iodohydrinohydride (LiH * Br and LiH * I) were reacted with hydrogen with 1 g of Li and 0.5 g of LiNH ₂ (Alfa Aesar, 99% Were synthesized. The compound was prepared in a stainless steel gas cell (Fig. 4) to contain further Raney Ni (15 g) (WR Grace Davidson) as a hydrogen dissociation agent according to the aforementioned method [13-14]. The reactor was operated with addition of hydrogen for 72 hours at 500 ° C in a kiln, and the pressure was cycled between 1 Torr and 760 Torr. The reactor was then cooled under helium gas. A sealed reactor was opened in the glove box under argon gas. The NMR sample was placed in a glass ampoule, sealed with a rubber stopper, and moved out of the glove box to make it incontinent. ¹ H MAS NMR was performed on LiH * X (X is a halide) solid sample as previously described [13-14] (Spectral Data Services, Inc., Champaign, Illinois). Chemical shifts were referenced to external TMS. In addition, XPS was performed on a crystal sample treated as an air-sensitive substance.

Since the synthesis reaction involved LiNH ₂ and Li ₂ NH 3 is the reaction product, both materials were used alone and as a control group in LiBr or LiI substrates. LiNH ₂ is a commercially available starting material, and Li ₂ NH is synthesized by the reaction of LiNH ₂ and LiH [67] and synthesized by the decomposition of LiNH _2. [68] Li ₂ NH, which is a product, (XRD). LiH (Aldrich Chemical Company, 99%), LiNH ₂ , and Li (Aldrich Chemical Co., Ltd.) Were used to eliminate the possibility that the alkali halide was affected by local quantum environments or produced NMR resonance, A control group containing the same molar ratio mixture of ₂ NH and LiX was utilized. Equimolar amounts of the compounds were mixed in a glove box under argon to prepare a control. The electron spin of the LiH * Br and LiH * I samples was carried out in such a way that it would not be possible to generate high field-shifted NMR resonance by eliminating F centers that are likely to provide a localized quantum environment of any known species. Resonance spectroscopy (ESR) was performed. For the ESR analysis, the sample loaded in a quartz tube (Suprasil) having a diameter of 4 mm and was reduced to a final pressure of 10- ⁴ Torr. The ESR spectra were recorded at room temperature and 77 K using an X-band spectrometer (Bruker, ESP 300). The magnetic field was calibrated using magnetic force gage (Varian, E-500 gauss meter). The microwave frequency was measured using a frequency meter (HP Company, 5342A).

Elemental analysis was performed (Galbraith Laboratories) to identify the resulting composition and eliminate the NMR detectability of transition metal hydrides or other hydrides that could generate high long-shift peaks. In particular, the presence of all the elements (Li, H, X) and all elements (Ni, Fe, Cr, Mo, Mn, Al) present in the R-Ni were analyzed.

NaH (3.28 g) and NaH (1 g) (Aldrich Chemical Company, 99%) were reacted with hydrogen as a raw material of the NaH catalyst and the corresponding alkali halide (15 g, NaCl or NaBr) (Alfa Aesar, ACS grade 99 +%) was reacted with intrinsic atom H to synthesize NaH * Cl and NaH * Br. Platinum-plated titanium mini-expanded cathode, 0.089 cm x 0.5 cm x 2.5 cm, platinum layer 2.54 mu m) as the hydrogen dissociation agent, and Pt / Ti (Pt coated Ti (15 g); Titan Metal Fabricators Co., (Fig. 4). &Lt; / RTI &gt; Each synthesis was carried out according to the method described for Li except for the kiln maintained at 500 ° C. The effect of using NaH (s) as a single hydrogen source was measured by repeated synthesis of NaH * Cl without addition of hydrogen gas . Since there are no possible element peaks in the region of H ^- (1/4), XPS was performed on NaH * Cl and NMR spectroscopy was performed on both products.

In addition, NaH * Cl, the only source of hydrogen, was synthesized from NaCl (10 g) and KHSO ₄ (1.6 g) as a solid using a kiln maintained at 580 ° C. Because the high concentration of H in the dissociation with H ₂ or a hydride, H according to the equation 27 ^- in the case where fast response to (1/4) partially inhibited, by the reaction of Equation 23 to H 25 ^- (1 / 3) could be formed.

Silicon wafers (2 g, 0.5 x 0.5 x 0.05 cm, Silicon Quest International, silicon (100), boron-doped, heated to 700 ° C under vacuum) were treated with Na (1.7 g), NaH 10 g), and Pt / Ti (15 g) and coated with the products NaH * Cl and NaH *, where NaCl was initially heated to 400 ° C under vacuum to form H ₂ (1 / 4) were removed. The reaction was carried out at 550 ° C in a kiln for 19 hours at an initial hydrogen pressure of 760 Torr. XPS was performed using a silicon wafer (NaH * -coated Si) coated with only sodium hydrinohydride. NaH * Cl-coated silicon wafers (NaH * Cl-coated Si) were analyzed by electron beam excitation spectroscopy. In addition, the emission spectrum of the pressurized pellet of the NaH * Cl crystal was recorded.

ToF-SIMS spectrum. A crystal sample of LiH * Br, LiH * I, NaH * Cl, NaH * Br, and a corresponding alkali halide control sample was spread on the surface of a double-sided adhesive tape, and a ToF- SIMS apparatus (Physical Electronics Co., TFS-2000) Respectively. The primary ion gun was a ⁶⁹ Ga + liquid metal source. ^Two (60 탆) areas of each sample were analyzed. To remove impurities on the surface and expose a clean surface, the samples were sputtered for 60 seconds using raster (180 [mu] m x 100 [mu] m). The gap setting was set to 3, and the ion current was set to 600 pA, and the total ion addition amount was set to 10 ¹⁵ ions / cm 2.

During capture, ion guns were activated using a 15 kV beam of bundle type (pulse width 4 ns packed in 1 ns) [69-70]. The total ion addition amount was 10 ¹² ions / cm 2. The charge was neutralized and the post-acceleration voltage was 8000 V. Positive and negative SIMS spectra were obtained. Representative late sputtering data was recorded.

In addition, 0.1 g of Na, 0.5 g of NaH, and 15 g of Pt / Ti were loaded into a water-flow calorimetry cell and water-flow calorimetry was performed under the same conditions as described for Na and R-Ni Respectively. While the cell produced an excess energy of 15 kJ, the theoretical energy balance obtained from the decomposition of NaH was an endotherm of about +1.2 kJ. Therefore, in order to confirm the presence of the hydrinohydride corresponding to the reaction given by Equation 23-25 as the source of excess heat, by the same procedure as for the crystal sample except for sputtering for 100 seconds, A sample of Pt / Ti coated with linolehydride (NaH * -coated Pt / Ti) was directly analyzed. Unreacted Pt / Ti was coated as a starting material and used as a control. XPS was also performed.

To F-SIMS of R-Ni 2400 which had been reacted at 50 캜 for 48 hours was carried out by the same procedure as for the crystal sample. The reaction to form hydrinos is given in equations 32-35. Because the surface was coated with NaOH, a sodium hydrinohydride composition with NaOH was predicted.

FTIR spectroscopy. FTIR spectroscopy with a DTGS detector at a resolution of 4 cm &lt;&quot; ¹ &gt; (Nicolet, Inc., Princeton University, New Jersey) was performed on the solid- 730) The procedure of use is as described above [13-14]). The samples were handled under inert gas. The resolution was 0.5 cm ^-1 . The control group LiNH _2, Li ₂ NH, and Li comprises a ₃ N, these are commercially available, but that of Li ₂ NH is by decomposition of LiNH ₂ and of the LiH react or [67] LiNH ₂ [68] And the Li ₂ NH 3 product was identified by X-ray diffraction (XRD).

XPS spectrum. A series of XPS analyzes were performed on the crystal samples using an XPD spectrometer (Scienta 300). The transmission mode of the analyzer and the sweep acquisition mode were used. The step energy in the general scan was 0.5 eV and the step energy in the high resolution scan was 0.15 eV. In a general scan, the step time was 0.4 seconds and the number of cathode sweeps was 4. In a high resolution scan, the step time was 0.3 seconds and the number of cathode lines was 30. C 1s at 284.5 eV was used as an internal standard.

UV spectroscopy of electron beam excited interstitial H ₂ (1/4). The lattice of the alkali halide (MgCl ₂ ) and the H ₂ (1/4) trapped in the silicon wafer were analyzed through electron impact of the crystal. Windowless UV spectroscopy of the electrons emitted from the electron beam excitation of the crystal at a beam preconditioning condition of 10 &lt; ^-5 &gt; Torr pressure of 10 &lt; ^-5 &gt; . The UV spectrum was recorded using a photomultiplier tube (PMT). The wavelength decomposition rate was about 2 nm (FWHM) when the entrance and exit slit width was 300 μm. The increment was 0.5 nm and the residence time was 1 second.

III. Results and Discussion

A. RT-Plasma Emission and Ballmer series α-line width.

Argon-hydrogen (95/5%) -lithium rt-plasma at a low temperature (e.g., 10 ³ K) condition of low field (1 V / cm) was obtained from LiNH ₂ vaporized by heating and atomic hydrogen produced in the titanium filament . Lithium and H-releasing electrons were detected, and LiNH ₂ used as a raw material for the atoms Li and H and Li as a decomposition product thereof were confirmed. Argon in the argon-hydrogen mixture increased the amount of atom H, which is evidenced by the apparent reduction of H emission in the absence of argon. H-Balmer series emitting electrons corresponding to a group with an energy level of > 12 eV were observed as shown in FIGS. 5 and 6, which also requires the presence of Lehman series emitting electrons.

Plasma is not formed by only argon / hydrogen. It is impossible for a titanium filament, vaporized LiNH ₂ , and a 0.6 Torr argon-hydrogen mixture to chemically react at a cell temperature of 700 ° C to account for the Ballmer series emitting electrons. In fact, there is no known chemical reaction that releases enough energy to excite the Ballmer series and Lehman series emitted electrons from hydrogen. In addition to known chemical reactions, electron impact excitation, resonant photon transition, and ionization and reduction of excitation energy by a " non-ideal " state in a strong plasma can also be used as an ionizing or exciting energy source to form hydrogen plasma Not suitable [21]. The energy required for the formation of the active reaction of atomic hydrogen satisfies the energy source that is liberated from the catalyst of atomic hydrogen by Li.

) 및 기기(

)에 따른 반진폭(half-width)으로부터 얻어진 각각의 가우시안 결과값의 총 반진폭(

)은 다음과 같다:The active hydrogen atomic energy was calculated using the width of the 656.3 nm Ballmer series α-ray emitted from the RF rt plasma. Doppler

) And equipment (

) &Lt; / RTI &gt; of each Gaussian result value obtained from the half-width according to

)Is as follows:

(40)

(40)

 Was ± 0.006 nm in this experiment. The temperature was calculated from the Doppler half amplitude using the following equation:

(41)

(41)

는 선 파장이고, T는 K (1 eV = 11,605 K)에서의 온도이며, μ는 분자량(원자수소=1로 함)이다. 각 경우에서, 평균 도플러 반진폭은 압력에 따라 쉽게 변하지 않았으나, ±10%의 에너지 오차에 대응하여 ±5% 범위에서 변화하였다.here,

T is the temperature at K (1 eV = 11,605 K), and μ is the molecular weight (atomic hydrogen = 1). In each case, the mean Doppler half amplitude did not change easily with pressure, but it varied in the range of ± 5% corresponding to an energy error of ± 10%.

For the argon-hydrogen (95/5%) -lithium rt-plasma, the Ballmer series alpha linewidth at 656.3 nm was recorded after the initial and 70 hour run, as shown in Figures 5A and 5B. The Bohrer series? Rays resulting from plasma emission at both viewpoints contain two separate Gaussian peaks, which contain an inner narrow peak corresponding to a slower component of less than 0.5 eV and an outer very corresponding to a fast component of greater than 40 eV It is a wide peak. The fast component reaches 90% of the initial n = 3 excited state H count and increases to 97% after 70 hours. Only hydrogen was widened. As we have seen, the energy source of the fast H is irrelevant to the added energy field and can be explained by the mechanism of the hydrogen catalyst in a low energy state. [32-37]

In addition, lithium rt plasma is formed at pure H ₂ gas at a pressure of 1 Torr, except at the initial and 70-hour points, only 27% of the population is about 6 eV in line width and number, 6A and 6B, respectively. This result was expected because excess H ₂ and Li could react with LiH to promote the collapse of LiNH ₂ as follows:

(42)

(42)

Therefore, the reaction to generate the atoms Li and H was weakened. Also, argon in an argon-hydrogen mixture can increase the amount of atomic hydrogen by preventing its recombination, and Ar ⁺ produced by the plasma can act as a catalyst, which is also the case with Li.

In the present invention, it is assumed that Doppler broadening due to heat change is the main reason and other cause factors are insignificant. This assumption has become clear when considering each causal factor. In general, the experimental design must take into account two Doppler effects, mechanical elements, natural elements (life span), Stark elements, van der Waals elements, resonance elements, and microstructures. The effect of each causative factor depends on the limit of detection [13-21, 38-39].

The formation of a fast H can be explained by the resonance energy transfer from a hydrogen atom to a Li atom, which is three times the potential energy of an atomic hydrogen, so that the central field is four times the proton, H &lt; * &gt; (1/4), which is the same number of intermediates as the hydrogen atom. Intermediates decrease spontaneously because of the rapid H (n = 1) reduction when the radius is reduced by collision or spatial energy transfer [27-29], which is also the case for previously reported photon emissions. Impact energy transitions involving through-space coupling are common. For example, the formation of H ₂ by a chemical exothermic reaction of H + H does not occur with the emission of photons. Rather, it collides with another entity M to remove the binding energy - [44]. The other entity distributes energy from the exothermic reaction to produce H ₂ and raise the temperature of the system. In the case of catalysis for the formation of the state given by equations 2a and 2c, the temperature of H is very high.

B. Differential Scanning Calorimetry (DSC). The DSC (100-750 ° C) of NaH is as shown in FIG. A broad endothermic peak was observed at 350 ° C to 420 ° C, corresponding to 47 kJ / mol. Sodium hydride is decomposed corresponding to an enthalpy of 57 kJ / mol over this temperature range [71]. Large exotherms were observed in the range of 640 ° C to 825 ° C, corresponding to -177 kJ / mol. The DSC (100-750 ° C) of MgH ₂ is as shown in FIG. Two distinct endothermic peaks were observed. The first peak was observed at 351.75 ° C, which corresponds to 68.61 kJ / mol MgH ₂ . Decomposition of MgH ₂ is the central part were observed at 440 ℃ to 560 ℃ corresponding to _{744 kJ / mol MgH 2 [71} ]. In Figure 8, the second peak was observed at 647.66 ° C, which corresponds to 6.65 kJ / mol MgH ₂ . The known melting point of Mg (m) is 650 ° C, which corresponds to a melting enthalpy of 8.48 kJ / mol Mg (m) [72]. Therefore, the expected result was observed in the decomposition process of the control non-catalytic hydride. On the other hand, the new heat development up to -177 kJ / mol NaH or at least -354 kJ / mol H ₂ or more, in the formula 23 to 25 through a given catalytic reaction was observed under the conditions of forming a catalyst with NaH part H. The observed enthalpy was greater than the enthalpy of almost all possible exothermic reactions for H, i.e., the hydrogen combustion enthalpy of -241.8 kJ / mol H ₂ .

는 에너지 공급량

및 임의의 초과 에너지

의 합과 동일해야 한다:C. Water - Flow rate calorimetry Power measurement. In each test, the energy supply and the energy release were calculated by the integral of the corresponding power. In the supplied power, the voltage and current measured at the end of each time interval were multiplied by the time interval (usually 10 seconds) to obtain the energy increase in Joule units. All energy gains were summed over the whole experiment after the equilibration period to obtain total energy. For energy emissions, the thermistor difference values were calculated after each test, assuming that the final values of inlet and outlet temperatures were the same. This difference value was calculated to be 0.036 ° C. The increase in the amount of heat energy due to the cooling water flow in each cycle was calculated using Equation 39, which is the water flow rate at 19 ° C (0.998 kg / liter), the specific heat of water (4.181 kJ / kg- ° C) , And time interval. The total energy release was obtained by combining the values throughout the entire experiment. Total energy of the cell

Energy supply

And any excess energy

Should be equal to the sum of:

(43)

(43)

From the energy balance equation, an excess calorific value was derived.

The results of the calibration test are shown in Figs. 10, there is a point at which the inclination of the cooling water power changes almost discontinuously. This time point of approximately one hour corresponds to a helium addition that improves the thermal transfer from the cell to the chamber walls. The numerical integration of the input and output power curves yields an output energy of 292.2 kJ and an input energy of 303.1 kJ, corresponding to a combination of 96.4% of the resistive input to the discharge chilled water.

The cell temperature and the chilled water power over time for the hydrinochemical reaction with a cell containing a sample containing Li as a catalyst material, 0.5 g of LiNH ₂ , 10 g of LiBr, and 15 g of Pd / Al ₂ O ₃ , 11 and 12, respectively. The numerical integration of the calibrated input and output power curves yields an output energy of 227.2 kJ and an input energy of 208.1 kJ. Therefore, from equation 43, the excess energy amount was calculated as 19.1 KJ. It can be seen from the diagram of FIG. 12 that there is a point where the slope of the temperature changes almost discontinuously. The change in slope occurs after one hour, which corresponds to a rapidly increasing cell temperature with the initiation of the reaction. Based on the system response to the power pulse, an excess of energy of 19.1 kJ occurred within two minutes when the power for the reaction was greater than 160 W. [

Quantitative XRD analysis of the composition produced in the reaction showed that LiBr and Pd / Al ₂ O ₃ did not change. Therefore, assuming 100% yield, the maximum of the theoretical energy value emitted from known compounds is 4.3 kJ, which is calculated according to equation 22 from the formation of lithium nitride and hydride, whereas the derived energy balance The value reached 4.4 times the above maximum value. Only exothermic reactions that can explain the energy balance are given in equations 17-19. The hydrogen content in 0.5 g of LiNH ₂ was 22 mmol H ₂ . Therefore, the derived energy balance is -870 kJ / mol H ₂ , assuming a maximum possible H ₂ list, which is more than 3.5 times the combustion energy of the most active hydrogen reaction, -241.8 kJ / mol H ₂ .

The cooling water power over time in the R-Ni power test with a cell containing a sample containing 15 g of R-Ni / Alalloy powder as a starting material for R-Ni and 3.27 g of Na 13 and 14, respectively. The curve for temperature and cooling water power time is very similar to the correction value. Through the numerical integration of the input and output power curves applying the correction values, an output power value of 384 kJ and an input power value of 385 kJ were calculated. Energy balance was obtained.

The cell temperature over time and the cooling water power over time in the hydrino reaction with a cell containing a sample containing 15 g of NaOH-doped R-Ni as a catalytic material, and 3.28 g of Na are shown in Figs. 15 and 16, respectively Same as. Through numerical integration of the input and output power curves with the correction values applied, an output energy of 185.1 kJ and an input energy of 149.1 kJ were calculated. Therefore, from equation 43, the excess energy amount was calculated as 36 kJ. It can be seen from the diagram of FIG. 15 that there is a point where the inclination of the temperature changes almost discontinuously. This change in slope occurs from 1 hour before, which corresponds to a rapidly increasing cell temperature with the initiation of the reaction. Based on the system response to the power pulse, an excess energy of 36 kJ occurred within 1.5 minutes when the power for the reaction was greater than 0.5 kW.

[75] 및

[65])이다. As a result of quantitative XRD analysis of a composition composed of NaOH-doped R-Ni reactant and reaction product with an alkali metal, it was found that Ni having a trace amount of Bayerite and Ni having a trace amount of alkali hydroxide Respectively. Reaction with sodium -Ni alloy formation or Ni-Al ₂ O ₃ and R of the sodium in the [73-74] is clear endothermic reactions (each

[75] and

[65]).

[65, 76])은, 초기의 미량의 배이어라이트 및 Na와의 반응으로부터 생성되는 NaOH를 보여주는 XRD 분석에 기초하여, 에너지 균형값에 거의 영향을 미치지 않음을 알 수 있다. 문헌 [74]에 나타난 바와 같이, 배이어라이트 분해물 내의 H₂O 함량은 47.7 μmole H₂O/g R-Ni이며, 이는 Al(OH)₃의 분해 (

)에 기인한 NaOH의 형성 (

[65])에 의해 거의 영향을 미치지 않는 것이다. 전체 반응은 배이어라이트와 나트륨이 반응하여 NaOH를 형성하는 것이다 (

).When forming heat, the formation of NaOH through the reaction of Bayerite with sodium (

[65, 76]) shows little effect on the energy balance value, based on XRD analysis showing NaOH generated from the initial trace amounts of valerate and reaction with Na. As shown in the literature [74], the H ₂ O content in the Baillardite degradation product is 47.7 μmole H ₂ O / g R-Ni, which is the decomposition of Al (OH) ₃

) Formation of NaOH (

[65]). The overall reaction is the reaction of the baileite with sodium to form NaOH (

).

An exothermic reaction that can account for the energy balance is given in equations 23-25. The hydrogen content of R-Ni was determined to be 150 μmole H ₂ / g R-Ni using the quantitative GC analysis and the ideal gas law of P, V, and T states. Therefore, the energy balance derived is -1.6 × 10 ⁴ kJ / mol H ₂ , assuming a maximum possible H ₂ list, and 66 times the combustion enthalpy of the most active hydrogen-241.8 kJ / mol H ₂ Over. Theoretical retention energy value calculated for the reaction of Equation 44 is 259 eV / H ₂ or _{25 mJ / moleH 2 [7]} .

(44)

(44)

The most active of the oxidation reactions involving solid fuels is known to have a combustion heat of 24 kJ / g and there is little known fuel / oxidant system producing more than 10 kJ / g [65]. In comparison, even if not completed, H contained in renewable catalyst NaH produced 300 times more energy than the energy per unit weight of the well-known solid fuel.

By increasing the NaOH doping and converting to R-Ni 2400, the catalytic material produced high power and energy without the need to add Na. The cell temperature and the chilled water power over time for the hydrinocne reaction with the cell containing 15 g of NaOH-doped R-Ni 2400 as catalyst are as shown in Figs. 17 and 18, respectively. The numerical integration of the input and output power curves with the correction value yields an output energy of 195.7 kJ and an input energy of 184.0 kJ, corresponding to an excess energy of 11.7 kJ and a power exceeding 0.25 kW.

Analysis of the product after the reaction with the composition of NaOH-doped R-Ni, which is a reactant, was analyzed by quantitative XRD, and it was found to be R-Ni and R-Ni having 3.7 wt% Was times followed by a H ₂ O content measured by the light decomposition of the initial R-Ni is 32.8 μmole, which _{3 wt% Al (OH) 3} - the ship after the H ₂ O content measured from the light degradation of the doped Ni / Al alloy 34.0 μmoles H ₂ O / g. Most possible exothermic reactions were from Al (OH) ₃ to Al ₂ O ₃ . The equilibrium equation is given by [65, 75, 77]:

(45)

(45)

이다. 이는 3 wt% Al(OH)₃-도핑된 Ni/Al 알로이 15g의 열측정에 의해 확인되었는데, 상기 열측정에서 평균 에너지는

로 나타났으며, 이는 이론적인 에너지값인

과 비교되는 값이다 (식 45 에서

일 때

[75]). 그러므로, NaOH-도핑된 R-Ni로부터 관찰된 에너지는 이론값의 4.4배였으며 이는 식 23 내지 25에서 주어진 촉매 반응에 더 많은 영향을 줄 수 있었다.* In 3.7 wt% Al ₂ O ₃ , the maximum theoretical energy in the reaction given by equation 45 is

to be. This was confirmed by the thermal measurement of 15 g of a 3 wt% Al (OH) ₃ -doped Ni / Al alloy,

, Which is the theoretical energy value

(Equation 45) &lt; RTI ID = 0.0 &gt;

when

[75]). Therefore, the energy observed from the NaOH-doped R-Ni was 4.4 times the theoretical value, which could have had a greater effect on the catalytic reaction given in equations 23-25.

D. ToF-SIMS spectrum. Positive ToF-SIMS spectra obtained from LiBr and LiH * Br crystals are shown in Figures 19 and 20, respectively. The positive ion spectra of LiH * Br crystals and LiBr control were mainly Li ⁺ ions. Other Li ₂ ⁺ , Na ⁺ , Ga ⁺ , and Li (LiBr) ⁺ were also observed.

The anion ToF-SIMS of LiBr and LiH * Br crystals is as shown in Figs. The H ^- and Br ^- peaks were mainly observed in the LiH * Br spectrum and the intensity was H ^- > Br ^- . In the anion ToF-SIMS of LiBr control group, only bromine ion was mainly observed. In both cases, O ^- , OH ^- Cl ^- , and LiBr ^- were also observed. In addition to the increased hydride, LiHBr &lt; ^- &gt; and Li ₂ H ₂ Br ^- , which satisfy the formation of new lithium borohydride as another characteristic peak of the LiH * Br sample, were observed.

)을 도 27에 나타내었다. 일련의 하이드리노-하이드라이드-화합물인 NaH_x ^-도 관찰되었는데, 이 때 고성능 (10,000) 질량 결정법으로부터 얻은 질량 손실량을 통해 대조군에서 관찰된 일련의 C₂H_x ^-에 대한 이의 작용을 명확히 알 수 있었다. XPS 스펙트럼에 따르면 NaH*-코팅된 Pt/Ti는 두 개의 수소 상태, 즉 H^-(1/3) 및 H^-(1/4)을 포함하고 있다 (Sec. IIIF).Positive ToF-SIMS spectra obtained from LiI and LiH * I crystals are shown in Figures 23 and 24, respectively. In the positive ion spectra of LiH * I crystals and LiI control, Li ⁺ ions were mainly observed. Li ⁺ , Na ⁺ , Ga ⁺ , and a series of positive ions Li [LiI] _n ⁺ were also observed. The characteristic peaks of the LiH * I sample are LiHI +, Li ₂ H ₂ I ⁺ , Li ₄ H ₂ I ⁺ , Li ₆ H ₂ I ⁺
Anions ToF-SIMS of LiI and LiH * I crystals are shown in Figures 25 and 26, respectively. In the LiH * I spectrum, H ^- and I ^- peaks were mainly observed, and the intensity was H ^- > I ^- . Iodine ion was mainly observed in anion ToF-SIMS for LiI control. In both cases, O ^- , OH ^- , Cl ^- , and a series of anions I [LiI] _n ^- were observed together. In addition to the increased hydride, LiHI ^- , Li ₂ H ₂ I ^- , and NaHI ^- , which satisfy the formation of a novel lithium iodohydride, were observed as characteristic peaks of the LiH * I sample.
Negative ToF-SIMS spectra for NaH * -coated Pt / Ti with the generation of excess heat of 15 kJ (

) Is shown in Fig. A series of hydrino-hydride compounds, NaH _x ^- , were also observed, demonstrating their apparent action on the series of C ₂ H _x ^- observed in the control through mass loss from high-performance (10,000) mass determination there was. According to the XPS spectrum, NaH * -coated Pt / Ti contains two hydrogen states: H ^- (1/3) and H ^- (1/4) (Sec. IIIF).

delete

delete

Na / R-Ni water - In the spectrum of R-Ni obtained by water-flow calorimetric analysis, NaH _x ^- with a series of mass defects was found to produce 36 kJ of excess heat. The positive ToF-SIMS spectrum obtained from R-Ni reacted at 50 占 폚 for 48 hours is shown in Fig. The main ion on the surface was Na ⁺ along with doped NaOH on the surface. Ions of other major elements of R-Ni 2400 such as Al ⁺ , Ni ⁺ , Cr ⁺ , and Fe ⁺ were also observed.

과의 결합이온에 해당한다. 그 외 관찰되는 다른 특징적인 피크는 NaOH, NaO, OH- 및 O^-과 결합된 소듐 하이드리노 하이드라이드 NaHx-에 해당한다.Fig. 29 shows the ToF-SIMS result of anion of R-Ni reacted at 50 DEG C for 48 hours. In the spectrum, OH ^- and O ^- hydroxyl radicals were observed along with a very large H ^- peak. Two other major peaks correspond to a high resolution mass of 10,000, NaH ₃ ^- and NaH ₃ NaOH ^- which corresponds to the sodium hydrinohydride and its

And the like. The other characteristic peaks are observed outside is NaOH, NaO, OH- and O ^- corresponds to the sodium hydride hydroxy Reno NaHx- combined with.

^{E. H - (1/3), H} -. (1/4), H 2 (1/3) , and H ₂ (1/4 NMR identification of LiH with a relative value to external TMS * Br and LiH * I of each was shown a ¹ H MAS NMR spectrum is shown in Fig. 30A and 30B. LiH * X samples showed very high high field (upfield) resonance corresponding to each X = Br, and X = I at -2.51 ppm and -2.09 ppm . was LiH, a mixture of LiH and LiBr or LiI in the same molar ratio, LiNH _2, Li ₂ NH, and none of the high section of the control group containing LiNH ₂ or Li ₂ NH and a mixture of LiBr or LiI in the same molar ratio - change peak Since the high long peak of LiH * X at about -2.2 ppm is very large, it is better to compare these results with the identification results of H ^- (1/4) of KH * Cl and KH * I .

The TMS and relative ¹ H MAS NMR spectra (FIG. 31A) for the KH * Cl samples from individual syntheses and controls were described above [13-15, 24-26]. The experimental absolute resonance shift of TMS is -31.5 ppm compared to the rotating magnetic frequency of both [78-79]. The experimental shift value of KH with reference to TMS is +1.1 ppm, corresponding to an absolute resonance shift of -30.4 ppm, and the expected shift value of H ^- (1/1) calculated by Equation 4 for p = 0 -30 ppm. The shift value of the new peak for TMS is -4.46 ppm, which corresponds to an absolute resonance shift value of -35.96 ppm, and p = 4 in Equation 4. H ^- (1/4) is the hydride ion predicted using K as a catalyst [1, 15, 30]. In addition, a very narrow peak width refers to a small hydride ion that is a free rotor. In contrast, in the case of KH * I (FIG. 31B), a very wide peak appears at -2.31 ppm. KH I * of the expected product hydride ions H of the reaction with the catalyst K to form a ^- (1/4) was observed at 11.2 eV of the binding energy thereof estimated by XPS [13-15, 26, 30] . Therefore, the hemispherical migration due to the large halide ion is +2.15 ppm. The corrected high peak NMR peaks for LiH * X are each about -4.46 ppm, which is consistent with the expected migration values of the free ions given by Equation 4.

As a result of elemental analysis in terms of weight% of LiH * Br, Li (8%), H (1.1%) and I (90.9%) were obtained. This is because the stoichiometric ratio of detectable LiHBr in stainless steel and R- Is the corresponding value. Li (5.2%), H (0.8%) and I (94%) were obtained by elemental analysis in terms of% by weight of LiH * I, indicating that the stoichiometric ratio of LiHI detected in stainless steel and R- Is the corresponding value. Therefore, other hydrides other than Li hydride are not applicable. UH does not have a high field-mobile NMR peak [13-14] as before. F center can not be the cause because there is no detectable ESR signal at LiH * Br or LiH * I at room temperature or 77 K. In the ¹ H MAS NMR spectra obtained from LiNH ₂ , Li ₂ NH, and compounds thereof in LiBr or LiI base, none of these compounds with high long-shifted NMR peaks appeared. To further remove LiNH ₂ and Li ₂ NH, which are the causes of the -2.5 ppm peak, a LiH * Br sample with a -2.5 ppm peak was heated to 600 ° C under dynamic vacuum to decompose LiNH ₂ and Li ₂ NH. The heat-treated samples were analyzed by FTIR spectroscopy and the results showed that the amides and imides were removed, which corresponded to the amide peaks at 3314, 3259, 2079 (wide peak), 1567, and 1541 cm ^-1 and the imide peak The peak at 3172 (wide peak), 1953, and 1578 cm ^-1 was found not to be found, and the -2.5 ppm peak was reanalyzed by NMR. The FTIR spectrum shown in Figure 45B shows that these species have been removed and the corresponding NMR spectrum showed a -2.5 ppm peak. Past and present NMR and FTIR analyzes showed that the -2.5 ppm peak in the ¹ H NMR spectrum was not associated with UH, LiNH ₂ , Li ₂ NH, or other known species, and the -2.5 ppm peak in the ¹ H NMR spectrum was theoretical Corresponds to the anticipated H ^- (1/4) ion, confirming the direct evidence of hydride ion in the low-energy state.

In addition to the -2.5 ppm and -2.09 ppm peaks corresponding to H ^- (1/4), 1.3 ppm peaks were observed in the ¹ H MAS NMR spectra of LiH * Br and LiH * I, which are shown in FIGS. 30A and 30B, respectively . None of the controls showed this peak to remove the starting compound or possible known products. However, this peak may be due to the H ₂ (1/4) molecule corresponding to H ^- (1/4).

Through gas phase ¹ H NMR, H ₂ was analyzed. The experimental absolute resonance shift of gaseous TMS compared with the rotational frequency of both is -28.5 ppm [80]. H ₂ was observed at 0.48 ppm compared to the gaseous TMS set at 0.00 ppm [81]. Therefore, an absolute gas phase H ₂ 0 people moving value corresponding to -28.0 ppm (-28.5 + 0.48) ppm was exactly the same as the absolute value of the moving gas phase -28.01 ppm of expected given in Equation 12.

Absolute H ₂ gas phase shift values can be used to determine substrate shift values for H ₂ in a lithium-based substrate. Correction to the substrate migration value can then be compared to Equation 12 by adding a 1.3 ppm peak and determining the gas phase absolute migration value. The shift values of all the peaks were compared with the liquid phase TMS, which has an experimental absolute resonance shift of -31.5 ppm for the rotational magnetic frequencies of the two peaks. Experimental shift values of H _{2 in} the lithium compound base at 4.06 ppm with respect to the liquid TMS are shown in FIG. 7 (Lu and others) corresponding to the absolute resonance shift value of -27.44 ppm (-31.5 ppm + 4.06 ppm) do. And - (3.5 ppm 4.06 ppm), 3.5 ppm (-28.0 ppm - - 31.5 ppm) for the liquid when using the absolute TMS H ₂ gas phase 0 people movement of -28.0 ppm, a lithium compound corresponding to the substrate effect is +0.56 ppm This needs to be corrected to a measurement shift value of -0.56 ppm. The high long peak of H ₂ at 1.26 ppm peak to TMS then corresponds to a substrate-corrected absolute resonance shift of -30.8 ppm (-31.5 ppm + 1.26 ppm - 0.56 ppm). When we substitute the data in Equation 12, p = 4 and H ₂ (1/4) match:

(46)

(46)

에 대한 상대적인 강도가 증가된 것이다. 도 6 및 7에서 알려지지 않은 피크에 대해서는 확인할 수 없었다. H₂(1/4)의 이론적인 이동값과 정확히 일치하는 피크에 대한 확인은, FTIR (Sec. IIIG)과 전자 빔-여기 방출 분광법 (Sec. IIIH)에 의해 실시하였다.Lu et al. [82] observed a peak at this location as LiH + LiNH ₂ (1.1 / 1) was heated

And the relative strength to the &lt; RTI ID = 0.0 &gt; But could not be confirmed for the unknown peaks in Figures 6 and 7. Identification of peaks that exactly corresponded to the theoretical shift of H ₂ (1/4) was performed by FTIR (Sec. IIIG) and electron beam-excited emission spectroscopy (Sec.

The presence of H ^- (¼) ion in LiH * X was found through the polarization of halide ions. The ¹ H MAS NMR spectra of LiH * F and LiH * Cl are as shown in FIGS. 32A and 32B. The peaks at 4.3 ppm and 1.2 ppm corresponded to the theoretical predictions of molecular hydrogen in two different quantum states [1, 6]. 4.3 ppm was consistent with the prediction of Lu et al. [82] for H ₂ , and 1.2 ppm was consistent with H ₂ (1/4) not initiated by Lu et al. [82]. The presence of H ₂ (1/4) can be seen by observing the predicted value of the rotational transition in the FTIR spectrum (Sec. IIIG) and the expected value of the rotation distance by electron beam-excited emission spectroscopy (Sec. H ^- (1/4) was ion peak is the main peak in both LiH * Br and LiH * I other hand can not be found in the LiH * Cl I containing LiH * F and bipyeon polarized chlorine containing fluorine which is also polarized bipyeon 30A and 30B, respectively. These results polarization halide LiX and H ^- indicates that form a lithium hydride Hala Ido which correspond to the reaction of the (1/4) ion. Since the molecular species are trapped in the crystal lattice uniquely, the H ^- content selectivity of LiH * X to the molecular species bound to H ^- (1/4) ions alone or in combination with the polarizability of H ^- / 4). &Lt; / RTI &gt; The potassium catalyst formed H ₂ (1/4) very well but not in the KCl and KI substrates with H ^- (1/4), as shown in Figures 31A and 31B.

The ¹ H MAS NMR spectrum of NaH * Br with reference to the external TMS is shown in Fig. NaH * Br showed a large and apparent high resonance at -3.58 ppm. None of the controls containing NaH or the same molar ratio mixture of NaH and NaBr showed a high long peak. High field peak of -3.58 ppm of NaH * Br but not large, does not clearly than in the case of KH * I substrate H within KH * I ^- not have a great effect as the previous case of identifying the (1/4) . Therefore, the measured shift value is directly compared to the expected theory that the peak is shifted to a lower slope due to the substrate effect. The experimental absolute resonance transfer of TMS is -31.5 ppm for the quantum rotational magnetic frequency [78-79]. A new peak at -3.58 ppm for TMS corresponds to an absolute resonance shift of -35.08 ppm, which implies p = 4 in Equation 4. H ^- (1/4) is the expected preferred hydride ion when using the catalyst NaH (Equations 3-4 and 23-27). Similar to the case of LiH * X, the 4.3 ppm peak shown in Figure 33 corresponds to H ₂ , and the 1.13 ppm peak corresponds to H ₂ (1/4). The latter is generally observed as a desirable catalytic molecular product [29].

The NaH * Cl ¹ H MAS NMR spectrum with reference to the external TMS showing the effect of hydrogenation on the relative intensities of H ₂ , H ₂ (1/4), and H ^- (1/4) is shown in FIGS. 34A-34B . The addition of hydrogen H ^- thereby increasing the (1/4) peak and reduce the H ₂ (1/4) as the H ₂ is increased. To 1.1 ppm corresponding to the (1/4) high field peak moves, H ₂ (1/4) of the -4 ppm corresponding to the peak, and _{^{H 2 - (A) NaH *}} Cl H is synthesized by hydrogenating Shows the corresponding main peak of 4 ppm. (B) NaH * Cl H is synthesized without hydrogen addition ^- to the main peak, and H ₂ of 1.0 ppm for the (1/4) high field peak, H ₂ (1/4) of the -4 ppm corresponding to The corresponding small peak of 4.1 ppm is shown.

The effect of hydrogenation on the relative ¹ H MAS NMR of H ₂ , H ₂ (1/4), and H ^- (1/4) in NaH * Cl is shown in FIGS. 34A and 34B. With H ₂ (1/4) in H ₂ with the addition of external hydrogen is the main peak is converted to H ₂ is the space within the grid is filled by the H ₂ (1/4) H ₂ is occupied when not in abundance . However, the addition of hydrogen increases the relative intensity of the H ^- (1/4) peak, which may be due to the increased concentration of hydrinot reactant.

H quick reaction of the (1/4) which was partially inhibited in the case, the formation reaction of the formula 23 to 25 ^{- -} Since the high-concentration H is obtained by dissociation of H ₂ or a hydride not H according to equation 27 (1 / 3), the NMR was performed on NaH * Cl synthesized from KHSO ₄ solid acid, the sole source of NaCl and hydrogen. The ¹ H MAS NMR spectrum of the NaH * Cl formed using the solid acid with reference to the external TMS was shown in FIG. The peaks at -3.97 ppm and 1.15 ppm corresponded to peaks at -4 ppm and 1.1 ppm in Figures 34A and 34B, which correspond to H ^- (1/4) and H ₂ (1/4), respectively, Derived from NaH * Cl synthesized using H ₂ and H obtained by dissociating the hydride. Since the content of KHSO ₄ in the mixture with NaCl was only 6.5 mol%, a precise analysis was carried out so that the substrate effect was always constant between the samples. Specifically, peaks at -3.15 ppm and 1.7 ppm were observed in the solid acid product. As a result of using the above substrate shift values for NaH * Cl in equations 4 and 12, these peaks corresponded to H ^- (1/3) and H ₂ (1/3), respectively. Curve fitting of two peaks resulted in peaks at about -3 ppm and -4 ppm, which are theoretical values taking experimental error into account. H ₂ peaks therefore did not appear at 4.3 ppm, due to the synthesis of NaH * Cl with the solid acid, the sole source of H, and they are given by the equations 23 to 30 Confirm the reaction. The presence of H ₂ (1/4) and H ^- (1/4) in NaH * Cl obtained from the reaction of NaCl with solid acid KHSO ₄ was confirmed by XPS and electron beam-excited emission spectroscopy.

로의 전이 반응을 유발할 수 있는 다른 촉매이며, 이는 이차 이의 이온화에너지가 54.4 eV, (

)이기 때문이다. 촉매 반응은 다음과 같다:Helium

Is another catalyst capable of inducing a transition reaction to the secondary ion, which has an ionization energy of 54.4 eV, (

). The catalytic reaction is as follows:

(47)

(47)

(48)

(48)

And the overall reaction is as follows:

(49)

(49)

의

로의 순차적인 빠른 전이는, 식 27에서 주어진 바와 같이

에서 일차적으로 27.2 eV을 받아들이는 원자 수소에 의한 추가적인 촉매 반응을 통해 일어날 수 있다. 46.5 nm에서 시작되고 짧은 파장으로 이어지는 특징적으로 넓은 방출선은 활발한 H 촉매 분해로 인한 전이 반응 때문인 것으로 예상할 수 있다. 2% 수소를 갖는 헬륨의 마이크로파 방출을 기록하는 EUV 분광법을 이용하여 방출선을 관찰하였다[27-29]. 분광분석 및 NMR 데이터를 통해

의 형성과

으로의 순차 전이의 촉매 메카니즘을 확신할 수 있다. 추가적인 증거로서는 Sec. IIIF에서 주어진 바와 같이 NaH*Cl 내에서 H^-(1/3) 및 H^-(1/4) 모두가 관찰되는 것이다. As can be seen in the case of the NaH catalytic reaction, the He + catalyst product

of

The sequential rapid transition to &lt; RTI ID = 0.0 &gt;

Can be caused by an additional catalytic reaction by atomic hydrogen that accepts 27.2 eV first. The characteristic broad emission line starting at 46.5 nm and leading to a short wavelength can be expected to be due to the transient reaction due to active H catalytic decomposition. The emission line was observed using EUV spectroscopy to record the microwave emission of helium with 2% hydrogen [27-29]. Through spectroscopic analysis and NMR data

And

Lt; RTI ID = 0.0 &gt; of the &lt; / RTI &gt; Additional evidence includes Sec. H ^- (1/3) and H ^- (1/4) are observed in NaH * Cl as given in IIIF.

영역에 걸쳐 각각의 LiBr 및 LiH*Br에 대한 스펙트럼 분석이 실시되었다 (도 36A 내지 36B). LiH*Br 결정과 LiBr 대조군 내에 존재하는 모든 원소를 결정하기 위해 주 원소 피크를 조사하였다. 스캔 결과, 다음 피크를 제외하고는 낮은 결합 에너지 영역 (도 37) 내에서 피크를 확인할 수 있는 원소는 존재하지 않았다: Li 1s (55 eV, LiBr과 비교하여 1 eV 낮게 이동), O 2s (23 eV), Br 3d_5/2 및 Br 3d_3/2 (각각 69 eV 및 70 eV), Br 4s (15 eV), 및 Br 4d (5 eV). 따라서, 이 영역에서 나타나는 다른 피크는 새로운 종일 수 밖에 없다. 도 37에 나타난 바와 같이, LiH*Br의 XPS 스펙트럼은 LiBr과 비교할 때 9.5 eV 및 12.3 eV에서 추가적인 피크를 가지는 점에서 차이가 있으나, 이는 다른 어떠한 주 원소 피크와도 관련된 것도 아니며

하이드라이드 이온과 일치하는 것이다 (식 4 및 16). 이들 피크를 알아보기 위하여 원자가-밴드 영역에서 피크를 가지는 원소에 대하여 문헌을 검색하였다. 현재 알려진 주원소 피크로서는 이를 확인할 수가 없었다. 그러므로, 알려진 원소에는 해당하지 않으며 다른 어떠한 주원소 피크에도 대응하지 않는 9.5 eV 및 12.3 eV 피크는, 두 개의 다른 화학적 환경에 존재하는 H^-(1/4)임을 알 수 있었다. 이러한 사실은 KH*I의 H^-(1/4)에 대하여 이전에 보고된 바와 매우 유사하다 [13-15, 26, 30].F. XPS identification of H ^- (1/4) and H ^- (1/3).

Spectral analysis was performed for each LiBr and LiH * Br throughout the region (Figures 36A-36B). The main element peaks were investigated to determine all the elements present in LiH * Br crystals and LiBr controls. As a result of the scan, there were no peaks in the low binding energy region (Figure 37) except for the following peaks: Li 1s (55 eV, 1 eV lower compared to LiBr), O 2s (23 eV), Br 3d _5/2 and Br 3d _3/2 (69 eV and 70 eV, respectively), Br 4s (15 eV), and Br 4d (5 eV). Thus, other peaks appearing in this region are only new species. As shown in Figure 37, the XPS spectrum of LiH * Br differs in that it has additional peaks at 9.5 eV and 12.3 eV, as compared to LiBr, but it is not related to any other elemental peaks

Lt; / RTI &gt; (equation 4 and 16). To investigate these peaks, the literature was searched for elements having peaks in the valence band region. We could not confirm this as a currently known main element peak. Therefore, the known elements have not the 9.5 eV and 12.3 eV peak does not correspond to any other primary element peaks, two different H present in the chemical ^environment was found to be (1/4). This fact is of KH H * I ^- is very similar to that described previously reported with respect to the (1/4) [13-15, 26, 30].

영역에 걸쳐 각각의 NaBr 및 NaH*Br에 대해 스펙트럼을 얻었다 (도 38A 내지 38B). NaH*Br 결정 및 NaBr 대조군 내에 존재하는 모든 원소를 결정하기 위해 주 원소 피크를 조사하였다. 그 결과, 다음 피크를 제외하고는 낮은 결합 에너지 영역에서 확인할 수 있는 원소가 없었다: Na 2p 및 Na 2s (30 eV 및 63 eV, NaBr과 비교하여 1 eV 낮게 이동), O 2s (23 eV), Br 3d_5/2 및 Br 3d_3/2 (각각 69 eV 및 70 eV), Br 4s (15.2 eV), 및 Br 4d (5 eV). 따라서, 이 영역에서 나타나는 다른 피크는 새로운 종일 수 밖에 없다. 도 39에 나타난 바와 같이, NaH*Br의 XPS 스펙트럼은 NaBr과 비교할 때 9.5 eV 및 12.3 eV에서 추가적인 피크를 가지는 점에서 차이가 있으나, 이는 다른 어떠한 주 원소 피크와도 관련된 것도 아니며

하이드라이드 이온과 일치하는 것이다 (식 4 및 16). 이들 피크를 알아보기 위하여 원자가-밴드 영역에서 피크를 가지는 원소에 대하여 문헌을 검색하였다. 현재 알려진 주원소 피크로서는 이를 확인할 수가 없었다. 그러므로, 알려진 원소에는 해당하지 않으며 다른 어떠한 주원소 피크에도 대응하지 않는 9.5 eV 및 12.3 eV 피크는, 두 개의 다른 화학적 환경에 존재하는 H^-(1/4)임을 알 수 있었다.

A spectrum was obtained for each NaBr and NaH * Br throughout the region (Figures 38A-38B). The main element peaks were investigated to determine all the elements present in the NaH * Br crystals and the NaBr control. As a result, there were no detectable elements in the low binding energy region except for the following peaks: Na 2p and Na 2s (30 eV and 63 eV, 1 eV lower compared to NaBr), O 2s (23 eV) Br 3d _5/2 and Br 3d _3/2 (69 eV and 70 eV, respectively), Br 4s (15.2 eV), and Br 4d (5 eV). Thus, other peaks appearing in this region are only new species. As shown in Figure 39, the XPS spectrum of NaH * Br differs in that it has an additional peak at 9.5 eV and 12.3 eV compared to NaBr, but it is not related to any other elemental peak

Lt; / RTI &gt; (equation 4 and 16). To investigate these peaks, the literature was searched for elements having peaks in the valence band region. We could not confirm this as a currently known main element peak. Therefore, the known elements have not the 9.5 eV and 12.3 eV peak does not correspond to any other primary element peaks, two different H present in the chemical ^environment was found to be (1/4).

NaBr 영역에 걸쳐 15 kJ의 초과 열의 생성에 따르는 각각의 Pt/Ti 및 NaH*-코팅된 Pt/Ti에 대해 스펙트럼을 얻었다 (도 40A 내지 40B). NaH*-코팅된 Pt/Ti 및 Pt/Ti 대조군 내에 존재하는 모든 원소를 결정하기 위해 주 원소 피크를 조사하였다. 그 결과, 다음 피크를 제외하고는 낮은 결합 에너지 영역 (도 41A 내지 41B) 내에서 확인할 수 있는 원소가 없었다: Pt 4f_7/2 및 Pt 4f_5/2 (각각 70.7 eV 및 74 eV), 및 O 2s (23 eV). NaH*-코팅된 Pt/Ti에 대해 Na 2p 및 Na 2s 피크가 31 eV 및 64 eV에서 관찰되었으며, 원자가 밴드는 단지 Pt/Ti에 대해서만 관찰되었다. 따라서, 이 영역에서 나타나는 다른 피크는 새로운 종일 수 밖에 없다. 도 42A 내지 42B에 나타난 바와 같이, NaH*-코팅된 Pt/Ti의 XPS 스펙트럼은 Pt/Ti과 비교할 때 6 eV, 10.8 eV, 및 12.8 eV 에서 추가적인 피크를 가지는 점에서 차이가 있으나, 이는 다른 어떠한 주 원소 피크와도 관련된 것도 아니며

및

하이드라이드 이온과 일치하는 것 H^-(1/4)임을 알 수 있었다. 6 eV 피크는 H^-(1/3)에 해당하였다. 그러므로, 이 영역에서 할라이드 피크의 부재하에서, 부분적인 수소 상태 (1/3 및 1/4)는 식 27에서 예상된 바와 같이 관찰되었다. 높은 결합 에너지에 기인한 원자가 밴드의 부재는 NaH*-코팅된 Pt/Ti의 하이드리노 하이드라이드의 선별을 또한 만족하였다.

Spectra were obtained for each Pt / Ti and NaH * -coated Pt / Ti following the generation of an excess of 15 kJ over the NaBr region (Figures 40A-40B). The principal element peaks were investigated to determine all the elements present in the NaH * -coated Pt / Ti and Pt / Ti controls. As a result, there were no _detectable elements in the low binding energy region (Figures 41A-41B) except for the following peaks: Pt 4f _7/2 and Pt 4f _5/2 (70.7 eV and 74 eV, respectively) and O 2s (23 eV). Na 2p and Na 2s peaks were observed at 31 eV and 64 eV for NaH * -coated Pt / Ti, and the valence band was observed only for Pt / Ti. Thus, other peaks appearing in this region are only new species. As shown in Figures 42A-42B, the XPS spectrum of the NaH * -coated Pt / Ti differs in that it has additional peaks at 6 eV, 10.8 eV, and 12.8 eV when compared to Pt / Ti, Nor is it related to the elemental peak

And

And H ^- (1/4), which is in agreement with the hydride ion. The 6 eV peak corresponds to H ^- (1/3). Therefore, in the absence of halide peaks in this region, partial hydrogen states (1/3 and 1/4) were observed as expected in Equation 27. [ The absence of a valence band due to high binding energy also satisfied the selection of the hydrinohydride of NaH * -coated Pt / Ti.

The results of NaH * -coated Pt / Ti are shown in Figure 42B, which is identical to the result of NaH * -coated Si. As shown in Figures 43 and 44, the XPS spectrum of NaH * -coated Si showed peaks at 6 eV, 10.8 eV, and 12.8 eV, which do not correspond to known elements and do not correspond to any other elemental peaks But it is in agreement with H ^- (1/3) and H ^- (1/4). Therefore, the partial hydrogen state 1/3 (H ^- (1/3) at 6 eV) and 1/4 (H ^- (1/4 at 10.8 eV and 12.8 eV) exist.

G. Identification of FTIR of H ₂ (1/4). High-performance FTIR for samples with high peak-shifted ¹ H NMR peak at -2.5 ppm corresponding to H ^- (1/4) and NMR peak at 1.3 ppm corresponding to corresponding H ₂ (1/4) Spectral analysis was performed. As seen in Figure 45B, a single narrow peak was observed at 1989 cm &lt;&quot; ^{1 &} gt ;. LiNH ₂ , Li ₂ NH, and Li ₃ N compounds are possible when starting materials and expected reactions are considered, but none of these compounds show peaks in the region of 1989 cm ^-1 . No other peaks were observed other than the peaks easily predicted by LiBr (Fig. 45A). All species that can be found in this area, such as heterologous materials such as azides, metal carbonyls, metaborate ions, have been thoroughly investigated. The azide and metal carbonyls were excluded because their spectral bands must be very large. The ToB-SIMS analysis showed that the total boron content was not detected at the ppb level, which is lower than the FTIR detection limit, and the boron isotope, 10 ^B (20 % NA) and ¹¹ B (80% NA).

Considering possible substrate effects, the peak at 1989 cm ^-1 (0.24 eV) was consistent with the theoretical expected value of 1947 cm ^-1 for H ₂ (1/4). As it can be seen from equation 14 to 15, a very large rotational energy of up to ⁴² times the typical hydrogen means the internuclear distance of H ₂ (1/4) corresponding to 1/4 of the H _2. Invasive H ₂ in silicon and GaAs is close to a free rotor showing a single rotational oscillation transition [83-87]. H ₂ is not only an FTIR activity but also a Raman activity, which is due to the induced dipoles due to interaction with the crystal lattice [83]. The crystal lattice can also influence the law of choice and allow for other prohibited transitions within H ₂ (1/4). Considering the substrate effect, having a peak of 1943 cm ^-1 and a relatively narrow peak width means that H ₂ (1/4) can freely rotate within the crystal and correspond to one-fourth of the normal hydrogen dimension Which means that it has a small size. Typical hydrogen shows a ratio of ortho-para to 3: 1 at a non-cryogenic temperature, while a single peak of H ₂ (1/4) formed in a synthesis condition has a relative nuclear spacing of 1/4, resulting in a stability of 64 Only the para type can be seen as it gets better. The 1989 cm ^-1 peak is the peak of para-H ₂ (1/4), since the resulting frequency corresponds to the 1989 cm ^-1 peak and hydrogen is the only element known to exhibit a single rotational oscillation transition in the solid matrix, Corresponds to a rotational transition of J = 0 to J = 1.

H. H ₂ (1/4) rotation UV spectrum by electron beam excitation. H ₂ trapped in the alkali halide lattice _{(1/4), MgX 2 (X} = F, Cl, Br, I), and _{CuX 2 (X = F, Cl} , Br) UV spectroscopy (UV spectroscopy windowless) a windowless , And the electron beam excitation state of the crystal was measured under a beam current of 10-20 및 and a pressure range of less than 10 ^-5 Torr using a 12.5 keV electron gun. In the case of alkali metals, only alkali chloride showed a peak expected by Eq. 14, and the intensity roughly coincided with the expected value as the intensity increased as the heat progressed to the bottom of one group element row. In all cases, Lehmanic alpha peaks and other peaks were removed by heating, and were not observed in UV. In the online mass spectrometer only hydrogen was recorded. A series of _{MgX 2 (X = F, Cl} , Br, I) and the compound of CuX ₂ (X = F, Cl, B ), the expected band was only detected only MgI _2, the catalyst in this case Mg ²⁺ . NMR for these crystals gave only show the H ₂ (1/4) peak at 1.13 ppm only of MgX ₂ with the relative intensities of F, Cl, Br, << I , which electron beam only MgI ₂ - here release Of the band.

(

는 최종 상태의 회전 양자수)를 갖는 회전 에너지 간격의 예상치인 0.241 eV (식 14; p=4)와 일치한다. H₂(1/4)는 자유 회전자이나, 자유 진동자는 아니며 이는 앞서 예를 든 실리콘 내의 침입형 수소 [83-87]의 경우와 유사하다. 5.73 eV의 측정 경사값은 8.25 eV (식 13)의 진동에너지(

) 예상치로부터 실리콘 내의 침입형 H₂의 백분율에 비하여 2배 정도 이동하였다. 후자의 경우에는, 자유 H₂의 진동 에너지가 4161 cm^-1인 반면, 실리콘 내의 진동 피크가 오르쏘 및 파라-H₂에 대응하여 3618 및 3627 cm^-1에서 각각 관찰된다 [83]. 전자의 경우에는 이동치가 약 30% 낮은데, 이는 분자 진동 모드가 결정 격자와 결합함에 따라 질량이 두드러지게 상승하기 때문인 것으로 볼 수 있다. The spectrum of the 100-350 nm region for an electron beam-excited CsCl crystal with trapped H ₂ (1/4) is shown in FIG. A series of equal lines was observed in the 220 to 300 nm region as shown in FIG. These lines roughly corresponded to the spacing and strength of the P branches of H ₂ (1/4) given in Eq. 14. P (2), P (3), P (4), P (5), and P (6) were observed at 226.0 nm, 237.0 nm, 249.5 nm, 262.5 nm, 277.0 nm, and 292.5 nm Respectively. The slope of the linear curve with respect to the energy of the peak is 0.25 eV as shown in Fig. 46, and has a fraction of 5.73 eV and a residual error sum of r ² < 0.0000. The slope

(

Corresponds to the expected 0.241 eV (Equation 14; p = 4) of the rotational energy interval with the number of rotational quantum states in the final state. H ₂ (1/4) is not a free rotor or a free oscillator, which is similar to the case of the interstitial hydrogen [83-87] in the silicon described above. The measured slope value of 5.73 eV is 8.25 eV (Equation 13)

) Estimates of the intrinsic H _{2 content} in silicon. In the latter case, the vibration energy of free H ₂ is 4161 cm ^-1 , while the vibration peaks in silicon are observed at 3618 and 3627 cm ^-1 , respectively, corresponding to ortho- and para-H ₂ [83]. In the case of the former, the moving value is about 30% lower, which is due to the remarkable increase in mass as the molecular vibration mode is combined with the crystal lattice.

Using equations 14 and 15 with a measured rotational energy interval of 0.25 eV, an inter-nuclear distance of 1/4 of the normal H ₂ nuclear intercept for H ₂ (1/4) is derived. Corresponding weak bands were observed from NaH * Br, and a stronger band was observed from NaH * Cl. Considering the latter case, the emission intensity was significantly increased by H ₂ (1/4) captured in the silicon substrate. A 100-550 nm spectrum of a NaH * Cl coated electron beam-excited silicon wafer with trapped H ₂ (1/4) is shown in FIG. Observations were roughly consistent with the spacing and strength of the P branches of H ₂ (1/4) given in Equation 14. P (2), P (3), P (4), P (5), and P (6) were observed at 222.5 nm, 233.4 nm, 245.2 nm, 258.2 nm, 272.2 nm, and 287.4 nm Respectively. The slope of the linear curve with respect to the energy of the peak is 0.25 eV, as shown in Fig. 47, with a slice of 5.82 eV and a residual error sum of r ² < 0.0000. Linearity is a characteristic of rotation, and the result is again equal to H ₂ (1/4). This technique is based on Secs. IIIE and IIIG, as well as the solid-state NMR and FTIR results. As already known, when KH * Cl with H ^- (1/4) by [13-14] NMR was projected onto an electron beam of 12.5 keV, electron beam excited alkali chloride, NaH * Cl-coated Si, and argon - Excited H ₂ (1/4) excitation emission similar to that observed in hydrogen plasma was observed [13-14]. It was also observed that the band corresponding to H ₂ (1/4) was removed from the KCl starting material by heating at high temperature. Then KH * Cl after the synthesis from the heat-treated KCl trapped in the lattices of KH KH * Cl * Cl is H ^- were observed in addition to the (1/4), which is HCl, NaH, K, and multiple catalyst such as Ar ⁺ Can generate H ₂ (1/4).

Experimental Reference

1. R. Mills, The Grand Unified Theory of Classical Quantum Mechanics October 2007 Edition, posted at http://www.blacklightpower.com/theory/bookdownload.shtml.

2. R. Mills, K. Akhar, Y. Lu, "Spectroscopic Observation of Helium- and Hydrogen-Catalyzed Hydrino Transitions", to be submitted.

3. R. L. Mills, " Classical Quantum Mechanics ", Physics Essays, Vol. 16, No. 4, December, (2003), pp. 433-498.

4. R. Mills, "Physical Solutions of the Nature of the Atom, Photon, and Their Interactions to Form Excited and Predicted Hydrino States", in press.

5. R. L. Mills, " Exact Classical Quantum Mechanical Solutions for One-Through Twenty-Electron Atoms ", Physics Essays, Vol. 18, (2005), pp. 321-361.

6. R. L. Mills, " The Nature of the Chemical Bond Revisited and an Alternative Maxwellian Approach ", Physics Essays, Vol. 17, (2004), pp. 342-389.

7. R. L. Mills, "Maxwell's Equations and QED: Which is Fact and Which is Fiction", in press.

8. R. L. Mills, "Exact Classical Quantum Mechanical Solution for Atomic Helium Predicts Conjugate Parameters from a First Time", submitted.

9. R. L. Mills, "The Fallacy of Feynman's Argumenton the Stability of the Hydrogen Atom According to Quantum Mechanics," Annales de la Fondation Louis de Broglie, Vol. 30, No. 2, (2005), pp. 129-151.

10. R. Mills, " The Grand Unified Theory of Classical Quantum Mechanics ", Int. J. Hydrogen Energy, Vol. 27, No. 5, (2002), pp. 565-590.

11. R. Mills, The Nature of Free Electrons in Superfluid Helium-a Test of Quantum Mechanics and a Review of its Foundations and Make a Comparison to Classical Theory, Int. J. Hydrogen Energy, Vol. 26, No. 10, (2001), pp. 1059-1096.

12. R. Mills, " The Hydrogen Atom Revisited ", Int. J. of Hydrogen Energy, Vol. 25, Issue 12, December, (2000), pp. 1171-1183.

13. R. L. Mills, J. He, Y. Lu, M. Nansteel, Z. Chang, B. Dhandapani, " Comprehensive Identification and Potential Applications of New States of Hydrogen ", Int. J. Hydrogen Energy, Vol. 32 (14), (2007), pp. 2988-3009.

14. R. Mills, J. He, Z. Chang, W. Good, Y. Lu, B. Dhandapani, "Catalysis of Atomic Hydrogen to Novel Hydrogen Species H - (1/4) and H 2 (1/4) as a New Power Source &quot;, Int. J. Hydrogen Energy, Vol. 32, No. 12, (2007), pp. 2573-2584.

15. R. Mills, P. Ray, B. Dhandapani, W. Good, P. Jansson, M. Nansteel, J. He, A. Voigt, "Spectroscopic and NMR Identification of Novel Hydride Ions in Fractional Quantum Energy States, an Exothermic Reaction of Atomic Hydrogen with Certain Catalysts ", European Physical Journal-Applied Physics, Vol. 28, (2004), pp. 83-104.

16. R. Mills and M. Nansteel, P. Ray, " Argon-Hydrogen-Strontium Discharge Light Source ", IEEE Transactions on Plasma Science, Vol. 30, No. 2, (2002), pp. 639-653.

17. R. Mills and M. Nansteel, P. Ray, "Bright Hydrogen-Light Source Due to Resonant Energy Transfer with Strontium and Argon Ions", New Journal of Physics, Vol. 4, (2002), pp. 70.1-70.28.

18. R. Mills, J. Dong, Y. Lu, " Observation of Extreme Ultraviolet Hydrogen Emission from Incandescently Heated Hydrogen Gas with Certain Catalysts ", Int. J. Hydrogen Energy, Vol. 25, (2000), pp. 919-943.

19. R. Mills, M. Nansteel, and P. Ray, "Excessively Bright Hydrogen-Strontium Plasma Light Source Due to Energy Resonance of Strontium with Hydrogen", J. of Plasma Physics, Vol. 69, (2003), pp. 131-158.

20. R. L. Mills, J. He, M. Nansteel, B. Dhandapani, "Catalysis of Atomic Hydrogen to New Hydrides as a New Power Source", International Journal of Global Energy Issues (IJGEI), Special Edition in Energy Systems, Vol. 28, Nos. 2/3 (2007), pp. 304-324.

21. H. Conrads, R. Mills, Th. Wrubel, " Emission in the Deep Vacuum Ultraviolet from a Plasma Formed by Incandescent Heating Hydrogen Gas with Trace Amounts of Potassium Carbonate ", Plasma Sources Science and Technology, Vol. 12, (3003), pp. 389-395.

22. J. Phillips, R. L. Mills, X. Chen, " Water Bath Calorimetric Study of Excess Heat in Resonance Transfer Plasmas &quot;, Journal of Applied Physics, Vol. 96, No. 6, pp. 3095-3102.

23. R. L. Mills, X. Chen, P. Ray, J. He, B. Dhandapani, "Plasma Power Source Based on a Catalytic Reaction of Atomic Hydrogen Measured by Water Bath Calorimetry", Thermochimica Acta, Vol. 406 / 1-2, (2003), pp. 35-53.

24. R. Mills, B. Dhandapani, M. Nansteel, J. He, T. Shannon, A. Echezuria, " Synthesis and Characterization of Novel Hydride Compounds ", Int. J. of Hydrogen Energy, Vol. 26, No. 4, (2001), pp. 339-367.

25. R. Mills, B. Dhandapani, M. Nansteel, J. He, A. Voigt, "Identification of Compounds Containing Novel Hydride Ions by Nuclear Magnetic Resonance Spectroscopy", Int. J. Hydrogen Energy, Vol. 26, No. 9, (2001), pp. 965-979.

26. R. Mills, B. Dhandapani, N. Greenig, J. He, " Synthesis and Characterization of Potassium Iodo Hydride ", Int. J. of Hydrogen Energy, Vol. 25, Issue 12, December, (2000), pp. 1185-1203.

27. R. L. Mills, P. Ray, " Extreme Ultraviolet Spectroscopy of Helium-Hydrogen Plasma ", J. Phys. D, Applied Physics, Vol. 36, (2003), pp. 1535-1542.

28. R. L. Mills, P. Ray, B. Dhandapani, M. Nansteel, X. Chen, J. He, "New Power Source from Fractional Quantum Energy Levels of Atomic Hydrogen that Surpasses Internal Combustion", J Mol. Struct., Vol. 643, No. 1-3, (2002), pp. 43-54.

29. R. Mills, P. Ray, " Spectral Emission of Fractional Quantum Energy Levels of Atomic Hydrogen from a Helium-Hydrogen Plasma and the Implications for Dark Matter ", Int. J. Hydrogen Energy, Vol. 27, No. 3, (2002), pp. 301-322.

30. RL Mills, P. Ray, " A Comprehensive Study of Spectra of the Bound-Free Hyperfine Levels of Novel Hydride Ion H - (1/2), Hydrogen, Nitrogen, and Air", Int. J. Hydrogen Energy, Vol. 28, No. 8, (2003), pp. 825-871.

31. R. Mills, " Spectroscopic Identification of a Novel Catalytic Reaction of Atomic Hydrogen and the Hydride Ion Product ", Int. J. Hydrogen Energy, Vol. 26, No. 10, (2001), pp. 1041-1058.

32. R. L. Mills, P. Ray, B. Dhandapani, R. M. Mayo, J. He, "Comparison of Excessive Balmer α Line Broadening of Glow Discharge and Microwave Hydrogen Plasmas with Certain Catalysts", J. of Applied Physics, Vol. 92, No. 12, (2002), pp. 7008-7022.

33. RL Mills, P. Ray, B. Dhandapani, J. He, "Comparison of Excessive Balmer α Line Broadening of Inductively and Capacitively Coupled RF, Microwave, and Glow Discharge Hydrogen Plasmas with Certain Catalysts," IEEE Transactions on Plasma Science, Vol. 31, No. (2003), pp. 338-355.

34. R. L. Mills, P. Ray, " Substantial Changes in a Microwave Plasma Due to Combining Argon and Hydrogen ", New Journal of Physics, www.njp.org, Vol. 4, (2002), pp. 22.1-22.17.

35. R. L. Mills, P. Ray, B. Dhandapani, "Excessive Balmer α Linear Broadening of Water-Vapor Capacitively Coupled RF Discharge Plasmas" Int. J. Hydrogen Energy, in press.

36. R. Mills, P. Ray, B. Dhandapani, "Evidence of an Energy Transfer Reaction Between Atomic Hydrogen and Argon II or Helium II as a Source of Excessively Hot H Atoms in RF Plasmas", Journal of Plasma Physics, 2006 ), Vol. 72, Issue 4, pp. 469-484.24.

37. J. Phillips, C-K Chen, K. Akhtar, B. Dhandapani, R. Mills, "Evidence of Catalytic Hydrogen in Hydrogen in Argon Plasmas", International Journal of Hydrogen Energy, Vol. 32 (14), (2007), 3010-3025.

38. R. Mills, P. Ray, R. M. Mayo, " CW HI Laser Based on a Stationary Inverted Lyman Population Formed from Incandescently Heated Hydrogen Gas with Certain Group I Catalysts ", IEEE Transactions on Plasma Science, Vol. 31, No. 2, (2003), pp. 236-247.

39. R. L. Mills, P. Ray, " Stationary Inverted Lyman Population Formed from Incandescently Heated Hydrogen Gas with Certain Catalysts ", J. Phys. D, Applied Physics, Vol. 36, (2003), pp. 1504-1509.

40. R. Mills, P. Ray, R. M. Mayo, " The Potential for a Hydrogen Water-Plasma Laser ", Applied Physics Letters, Vol. 82, No. 11, (2003), pp. 1679-1681.

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Claims (119)

delete delete delete delete delete delete delete delete delete delete delete delete delete delete delete delete delete delete delete delete delete delete delete delete delete delete delete delete delete delete delete delete delete delete delete delete delete delete delete delete delete Providing a reaction vessel constructed and arranged to contain pressures less than, equal to, or greater than atmospheric pressure; Providing a solid fuel mixture; Maintaining a pressure in a range lower than, equal to, or greater than atmospheric pressure; Providing a hydrogen atom in a reaction vessel from a first hydrogen atom source in communication with said reaction vessel; Providing a catalytic source of hydrogen atoms in communication with the reaction vessel, the reaction vessel comprising a reaction mixture of at least one reactant and at least one other element comprising elements or elements that form a catalyst so that a catalyst is formed from the source; Heating the reaction mixture to produce a catalyst of hydrogen atoms from a catalytic source of hydrogen atoms if the catalyst is not yet present or if the reaction to form the catalyst is not spontaneous at room temperature; If the reaction is not spontaneous at room temperature, the reaction mixture is heated to initiate the catalytic action of atomic hydrogen in the reaction vessel, whereby the catalytic action of atomic hydrogen releases an amount of energy greater than 300 kJ per mole of hydrogen &Lt; / RTI &gt; The reaction mixture (1) Na, NaH, NaNH _2, a source of sodium to NaOH, NaOH-coated R-Ni, NaX including (X is a halide), and NaX at least one of the R-coated Ni; (2) Al ₂ O ₃ , Pt, Ru, or Pd / Al ₂ O ₃ , R 2, Ni, Al, Sn, Al ₂ O ₃ , gamma, beta or alpha alumina, aluminate, sodium aluminate, alumina nanoparticles, O ₃ , carbon, Pt or Pd / C, inorganic compounds, Na ₂ CO ₃ , lanthanum oxide, M ₂ O ₃ , Si, silica, silicate, zeolite, Y zeolite powder, lanthanide element, transition metal, alkaline earth alloy with the alkali and Na, rare earth metals, SiO ₂ -Al ₂ O ₃ or SiO ₂ supported Ni, and other supported metal, an alumina-supported platinum, palladium, and ruthenium of which includes at least one of the at least one A support material having a large surface area support that aids in the production of NaH molecules from a source; (3) A source of hydrogen including H ₂ gas, dissociation agent and hydride, wherein the dissociation agent comprises Raney nickel (R-Ni), a valuable metal or a noble metal, a valuable metal or noble metal on the support, or a noble metal is at least one of Pt, Pd, Ru, Ir, and Rh, the support is Ti, Nb, Al ₂ O _3, SiO _2, and combinations thereof, on carbon Pt or Pd, the hydrogen spillover catalyst, a nickel fiber Pt, Pd, TiH, Pt black, and Pd black, refractory metals, molybdenum and tungsten, transition metals, nickel and titanium, internal transition metals, niobium, and the like, electroplated on a mat, a Pd sheet, a Ti sponge, And zirconium; a source of hydrogen; (4) a substituent comprising at least one of an alkali metal, an alkaline earth metal, an alkali metal hydride, and an alkaline earth metal hydride; (5) a metal source combined with a metal, an alkali metal, an alkaline earth metal, a lanthanide element, a transition metal, Ti, aluminum, B, a metal alloy, AlHg, NaPb, NaAl, LiAl and a metal sole or a second reducing agent, halide, transition metal halide, a lanthanide element halides, aluminum halides, metal hydrides, LiBH _4, NaBH4, LiAlH ₄ or NaAlH _4, and an alkali or alkaline earth metal and an oxidizing agent, AlX _3, MgX _2, LaX _3, CeX ₃ and TiX _n , and an Al intermetallic of R-Ni; a reducing agent for forming a NaH molecule; And (6) A method for producing power including R-Ni. 43. The method of claim 42, Wherein the catalyst of the hydrogen atom is at least one of the atoms Li, K or Cs. Providing a reaction vessel constructed and arranged to contain pressures less than, equal to, or greater than atmospheric pressure; Maintaining a pressure in a range lower than, equal to, or greater than atmospheric pressure; By providing a source of a catalyst of hydrogen molecules in communication with a reaction vessel comprising a solid fuel reaction mixture with at least one reactant and at least one other element comprising elements or elements that form a catalyst, step; And Heating the reaction mixture to produce a catalyst of hydrogen molecules from a source of the catalyst of the hydrogen molecule if the catalyst is not yet present or the reaction to form the catalyst is not spontaneous at room temperature; If the reaction is not spontaneous at room temperature, the catalytic action of the atomic hydrogen releases an amount of energy greater than 300 kJ per mole of hydrogen by heating the reaction mixture to initiate the catalytic action of atomic hydrogen in the reaction vessel &Lt; / RTI &gt; 45. The method of claim 44, Further comprising providing hydrogen atoms to the reaction vessel from a first source of hydrogen atoms in communication with the reaction vessel. 45. The method of claim 44, Wherein said catalyst is molecular NaH. 47. The method of claim 46, Further comprising reacting NaOH with a reducing agent to form molecular NaH in said reaction vessel. delete delete 45. The method of claim 42 or 44, Further comprising the step of removing the reaction product from the vessel and regenerating the source of the catalyst from at least a portion of the reaction product. 45. The method of claim 42 or 44, Further comprising the step of converting the emitted energy into electrical energy. 45. The method of claim 42 or 44, The source of the hydrogen catalyst comprises at least one reactant having hydrogen and at least one other element, Wherein the energy released is greater than the difference between the standard enthalpy of formation of the compound having the stoichiometry or the elemental composition of the product and the at least one reactant formation energy. 45. The method of claim 42 or 44, Wherein the source of the hydrogen catalyst comprises at least one reactant having hydrogen and at least one other element, Wherein the energy released is greater than the theoretical standard enthalpy required to regenerate at least one reactant from the product, wherein the energy to replace any reacted hydrogen to produce power is a standard value. 46. The method of claim 44 or 46, Further comprising preparing or regenerating the reaction mixture wherein at least one of the steps of mechanical mixing or separation, melting, filtration, hydrogenation, dehydrogenation, decomposition, evaporation, evaporation, vaporization and sublimation, and ball milling &Lt; / RTI &gt; delete delete delete 43. The method of claim 42, And X is Br or I. 43. The method of claim 42, M is selected from the group of La, Sm, Dy, Pr, Tb, Gd and Er. delete delete delete delete delete delete delete delete delete delete delete delete delete delete delete delete delete delete delete delete delete delete delete delete delete delete delete delete delete delete delete delete delete delete delete delete delete delete delete delete delete delete delete delete delete delete delete delete delete delete delete delete delete delete delete delete delete delete delete delete

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